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Sem 2- (6 week 1) Flashcards

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1
Q

Balance the following equation.

___Mg + ___O2 –>___MgO

2,2,2
2,1,2
1,1,2
The equation is already balanced.

A

2,1,2

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2
Q

If the reaction below begins with 5 grams of magnesium and produces 12 g of magnesium oxide, how much oxygen was used in the reaction?

____Mg + ____O2 –> ____MgO

7 g
17 g
60 g
2.5 g

A

7 g

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3
Q

Balance the following equation:

C2H4 + O2 –> CO2 + H2O

1, 1, 2, 2
1, 3, 2, 2
2, 6, 4, 4

A

1, 3, 2, 2

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4
Q

The equation is balanced: 2Fe + 3Cl2 –> 2FeCl3
True
False

A

True

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5
Q

The following equation is balanced: KI + Pb(NO­3)2 –> 2KNO3­ + PbI2
True
False

A

False

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6
Q

Balance the following equation by filling in the blanks.

H2SO4 + NaOH H2O + Na2SO4

A

1, 2, 2, 1

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7
Q

Which of the following represents the balanced the equation for the following reaction:

Hydrochloric acid reacts with lithium hydroxide to produce lithium chloride and water.

HCl + LiOH –> LiCl + H2O
HLi + ClOH –> LiOH + HCl
2HCl + LiOH –> LiCl + H2O
LiCl + H2O –> HCl + LiOH

A

HCl + LiOH –> LiCl + H2O

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8
Q

Balance the following equation by filling in the blanks.

MgBr2 + Fe­3P2–> Mg3P2 + FeBr2

A

3 MgBr2 + Fe­3P2–> Mg3P2 + 3 FeBr2

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9
Q

Balance the following equation by filling in the blanks.

CaCO3 + HCl –> CO2 + H2O + CaCl2

A

CaCO3 + 2 HCl –> CO2 + H2O + CaCl2

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10
Q

Balance the following equation by filling in the blanks.

Al2O3 + K –> K2O + Al

A

Al2O3 + 6 K –> 3 K2O + 2 Al

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11
Q

How many moles are in 34.4 g of water, H2O?

  1. 91 mol
  2. 02 mol
  3. mol
  4. 71 x 10^-23 mol
A

1.91 mol

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12
Q

How many grams are in 0.0430 moles of carbon dioxide, CO2?

  1. 000980 g
  2. 20 g
  3. 89 g
  4. 60 x 10^22 g
A

1.89 g

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13
Q

On average, a human being needs approximately 445 grams of O2 in a day. How many molecules of O2 are required to meet this requirement?

  1. 57 x 10^27 molecules
  2. 37 x 10^24 molecules
  3. 31 x 10^-23 molecules
  4. 67 x 10^25 molecules
A

8.37 x 10^24 molecules

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14
Q

How many moles are in 3.2 x 10^22 particles of K2CO3?

  1. 9 x 10^46 mol
  2. 4 x 10^24 mol
  3. 3 x 10^20 mol
  4. 053 mol
A

0.053 mol

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15
Q

A necklace is found to have 5.43 x 10^19 atoms of gold, Au. How many grams of gold are in the necklace?

  1. 0178 g Au
  2. 07 x 10^22 g Au
  3. 02 x 10^-5 g Au
  4. 44 x 10^45 g Au
A

0.0178 g Au

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16
Q

How many atoms of silver are in a ring with a mass of 4.5 grams?

  1. 042 atoms
  2. 7 x 10^24 atoms
  3. 9 x 10^26 atoms
  4. 5 x 10^22 atoms
A

2.5 x 10^22 atoms

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17
Q

How many moles are in 6.24 x 10^32 molecules of methane (CH4)?

  1. 00 x 10^34mol
  2. 89 x 10^31 mol
  3. 04 x 10^9 mol
  4. 78 x 10^56 mol
A

1.04 x 10^9 mol

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18
Q

How many moles will be needed if a chemist is trying to create 15.5 grams of K2SO4?

  1. 70 x 10^3 mol
  2. 0890 mol
  3. 33 x 10^24 mol
  4. 57 x 10^-23 mol
A

0.0890 mol

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19
Q

How many particles are in 0.00345 moles of CaCl2?

  1. 08 x 10^21 particles
  2. 73 x 10^-27 particles
  3. 383 particles
  4. 12 x 10^-5 particles
A

2.08 x 10^21 particles

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20
Q 
A jewelry factory has 1.23 moles of excess silver from the creation of a new bracelet. What is the mass of this excess silver?
  7.41 x 10^23 g
  2.04 x 10^-24 g
  133 g 
  0.0114 g
A

133 g

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21
Q

What are the coefficients for the equation below when it is correctly balanced?

Ca(OH)2 + HCl –> CaCl2 + H2O

1, 2, 1, 2
2, 1, 2, 1
1,2,1,1
1,1,1,2

A

1, 2, 1, 2

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22
Q

What is the correct coefficient for O2 when the following equation is correctly balanced?

C3H8 + O2 –> CO2 + H2O

3
5
4
1

A

5

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23
Q

If 53.5 g of C3H8 are burned in the presence of 15.0 g of oxygen to produce 23.3 g of CO2, how many grams of water will be produced?

C3H8 + O2 –> CO2 + H2O

  1. 8 g
  2. 2 g
  3. 2 g
  4. 8 g
A

45.2 g

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24
Q

What are the coefficients for the equation below when it is correctly balanced?

NaHCO3 + HC2H3O2–> NaC2H3O2 + CO2 + H2O

2, 1, 2, 1,1
1, 2,1,2,2
2, 1, 2,1,2
1,1,1,1,1

A

1,1,1,1,1

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25
Q

What is the correct coefficient for O2 when the following equation is correctly balanced?

Al2O3 –> Al + O2

4
3
2
1

A

3

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26
Q

What is the percent composition of an unknown hydrocarbon that is found to contain 21.7 grams of carbon and 4.85 grams of hydrogen?

What is the percent of Carbon?

  1. 9 %
  2. 1 %
  3. 5 %
  4. 5 %
A

81.9 %

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27
Q

Calcium carbonate (CaCO3) is a common ingredient found in antacids. What is the percentage of oxygen?

  1. 0 %
  2. 0 %
  3. 0 %
  4. 0 %
A

48.0 %

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28
Q

The percent of hydrogen in Al(OH)3 is ________.

Round your answer to three significant figures. Include only numbers in your answer.

A

Molar mass of Al(OH)3 = 26.98 + (3 mol O x 15.999) + (3 mol H x 1.008) = 78.001 g /mol

% H = [(3 mol H x 1.008) / 78.001] x 100 = 3.877%

Answer is 3.88%

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29
Q

The percent of carbon in methane (CH4) is ____.

  1. 9
  2. 1
  3. 1
  4. 5
A

74.9

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30
Q

Which compound has the highest percentage of oxygen?

Option	Compound
A	H­2O
B	CO2
C	NO2
D	C6H12O6

Option A
Option B
Option C
Option D

A

Option A

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31
Q

Butane is a gas commonly found in lighters. Butane has a formula of C4H10. Which of the following compounds is the correct empirical formula?

Option

Formula

A

C4H10

B

CH2

C

C2H5

D

CH

Option A
Option B
Option C
Option D

A

Option C

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32
Q

What is the empirical formula composed of 79g tin and 21g O?

A

Sn = 79 g / 118.71 g/mol = 0.665 mol Sn /0.665 = 1

O = 21 g /15.999 g/mol = 1.31 mol O / 0.665 =1.96 = 2

Answer: SnO2

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33
Q

An analyst determines the percent composition of a compound to be 82.8% carbon and 17.2% hydrogen. What is the empirical formula for this compound?

A

C = 82.8 g / 12.011 g/mol = 6.89 mol C / 6.89 = 1 x 2 = 2

H = 17.2 g / 1.008 g/mol = 17.06 mol H / 6.89 = 2.5 x 2 = 5

Remember, when the decimal ends in 0.5, you must multiply by 2 to make that a whole number.

Answer: C2H5

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34
Q

What is the molecular formula for an unknown compound with an empirical formula NO2 and a molar mass of 183.99 g/mol?

A

Empirical formula: NO2 Mass is 46 g/mol

N = 30.4 g / 14.007 g/mol = 2.17 mol N / 2.17 = 1

O = 69.6 g / 15.999 g/mol = 4.35 mol O / 2.17 = 2

Molecular mass / Empirical Mass = 183.99 / 46 = 4

4(NO2) = N4O8

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35
Q

What is the molecular formula for a compound containing 92.3% carbon and 7.7% hydrogen with a molar mass of 78 g/mol?

A

C = 92.3 g / 12.011 g/mol = 7.68 mol C / 7.63 = 1

H = 7.7 g / 1.008 g/mol = 7.63 mol H / 7.63 = 1

Empirical formula = CH

Molar mass / Empirical mass = 78/13 = 6

Multiply the empirical formula by a factor of 6

Answer: C6H6

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36
Q

An 85.16 g sample of a substance contains 28.95 g of copper, 12.77 g of nitrogen and the rest of the compound is oxygen. What percent of the compound is oxygen?

A

C: 28.95

N: 12.77

O: 43.43

Total: 85.16

%O = 43.4385.16 = 51.00%

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37
Q

What is the percentage of oxygen in sulfuric acid (H2SO4)?

A

H: 21.0082.016

S: 132.06532.065

O: 415.99963.996

Total = 98.077

% O= 63.99698.077100= 65.3%

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38
Q

The most common form of rust is iron (III) oxide. The formula for rust is Fe2O3. What percent of composition of iron in rust?

  1. 9%
  2. 1%
  3. 7%
  4. 3%
A

69.9%

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39
Q

Which of the following compounds has the highest percentage of carbon?

Option	Compound
A	C3H8
B	CH4
C	CO2
D	C6H12O6

Option A
Option B
Option C
Option D

A

Option A

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40
Q

An unknown molecule has a molecular formula of C24H48O24. What is the empirical formula?

Option	 Formula
A	C12H24O12
B	CH2O
C	C6H12O6
D	C8H16O8

Option A
Option B
Option C
Option D

A

Option B

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41
Q

A detective finds a body at an abandoned house that appears to have died due to an overdose of pain medication. The medication in the victim’s blood contains 71.56% carbon, 6.71% hydrogen, 4.91% nitrogen, and 16.82% oxygen. Use the data below to determine which pain medication caused the victim’s death.

Pain Medication

Empirical Formula

Codeine

C18H21NO3

Acetaminophen

C8H9NO2

Morphine

C17H19NO3

Demerol

C15H21NO2

Codeine
Acetaminophen
Morphine
Demerol

A

Morphine

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42
Q

Your lab partner has finished analyzing data and asks to compare his calculations with yours. While your data was collected together, you determined the empirical formula of your compound to be C2H4O3 and your partner argues that the correct empirical formula is C6H12O9. Is your partner drawing an accurate conclusion from the data you collected?
Yes because the elements are in the same ratio.
Yes because his conclusion shows the actual number of atoms in the molecule.
No because his formula is not in simplest terms.
No because your formula only shows the ratio, not the actual number of atoms in the molecule.

A

No because his formula is not in simplest terms.

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43
Q

A compound has an empirical formula of N2O and a molecular mass of 220 g/mol. What is the molecular formula for the compound?

A

N: 2 x 14.007 = 28.014

O: 1 x 15.999 = 15.999

Molar Mass of Empirical Formula: 44.013

22044.013=5

Molecular Formula is N10O5.

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44
Q

What is the molecular formula for a compound that is composed of 44.45 g of carbon, 3.73 g of hydrogen, and 51.82 g of nitrogen and a molecular weight of 81.09 g/mol. What is its molecular formula?

A

C: 44.45/ 12.011 = 3.70007/ 3.6996 = 1
H: 3.73/ 1.088 = 3.75984/ 3.6996 = 1
N: 51.82/ 14.007 = 3.6996/ 3.6996 = 1
Empirical Formula: CHN, Molar mass = 27.026 g/mol

81.0927.026=3

Molecular Formula is C3H3N3

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45
Q

A forensic scientist determines the percent composition of a hydrocarbon to be 65% carbon, 14% hydrogen and 21% oxygen. She also determines the molar mass of the compound to be 148 g/mol. She claims the molecular formula for the compound is C8H21O2. Is this a correct conclusion that can be drawn from the data? Be sure to explain your answer.

A

Yes because the molecular mass and the empirical formula established by the data match. Multiplying the molar mass of the hydrocarbon by each percent and then dividing the molar mass of the individual elements, should be approximately the numbers in the given empirical formula.

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46
Q

What is the ratio of chlorine gas to sodium chloride according to the following reaction:

2NaF + Cl2 –> 2NaCl + F2

A

When looking for the ratio, look at the coefficients in the balanced chemical equation. Also, make sure you record your answer in the order in which it was asked Cl2:NaCl

Answer: 1:2

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47
Q

Use the following equation to answer the question: 2NaF + Cl2 –>2NaCl + F2. If Xander is working in the lab and produce 6.25 moles of fluorine gas, how many moles of sodium chloride was also produced during this reaction?

  1. 13 mol NaCl
  2. 25 mol NaCl
  3. 5 mol NaCl
A

12.5 mol NaCl

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48
Q

What is the mole ratio of aluminum, Al to oxygen, O2 in the following equation:

4Al + 3O2 –> 2Al2O3

A

When looking for the ratio, look at the coefficients in the balanced chemical equation. Also, make sure you record your answer in the order in which it was asked Al:O2

4: 3

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49
Q

Using the same conditions from the previous reaction:

4Al + 3O2 –> 2Al2O3

How many moles of oxygen, O2 would be needed if Luis is looking to produce 2.75 moles of aluminum oxide, Al2O3?

  1. 83 mol O2
  2. 13 mol O2
  3. 06 mol O2
  4. 67 mol O2
A

4.13 mol O2

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50
Q

Using the same conditions from the previous reaction:

4Al + 3O2 –> 2Al2O3

How many moles of aluminum, Al would be needed if Susan is looking to use all of the 13.23 moles of oxygen, O2 available in the oxygen tank in the lab?

  1. 98 mol Al
  2. 820 mol Al
  3. 923 mol Al
  4. 64 mol Al
A

17.64 mol Al

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51
Q

What unit of measure is the key to performing stoichiometric calculations?
grams
moles
molar mass

A

moles

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52
Q

The decomposition of potassium chlorate (KClO3) is a relatively simple method by which to isolate oxygen gas (O2). How many grams of oxygen gas can be isolated from the decomposition of 2.12 moles of potassium chlorate according to the equation:

2KClO3 –> 2KCl + 3O2

67.8 g
50.9 g
102 g
45.2 g

A

102 g

53
Q

How many grams of KClO3 would Mark need if he is looking to isolate 155 grams of O2?

2KClO3 –> 2KCl + 3O2

396 g
890. g
594 g
12,600 g

A

396 g

54
Q

A standard lighter operates through the combustion of butane according to the reaction:

2C4H10 + 13O2 –> 8CO2 + 10H2O

How many grams of O2 are required to combust 0.534 grams of C4H10?

113 g

  1. 0607 g
  2. 972 g
  3. 94 g
A

1.94 g

55
Q

A standard lighter operates through the combustion of butane according to the reaction:

2C4H10 + 13O2 –> 8CO2 + 10H2O

How many grams of H2O are produced by the combustion of 0.789 mol of C4H10?

71.1 g
142 g
1.22 g
0.244 g

A

71.1 g

56
Q

Calcium carbonate (CaCO3) is a common ingredient in antacids. It works by neutralizing the hydrochloric acid in your stomach according to the following reaction:

CaCO3+ 2HCl –> CaCl2 + H2O + CO2

What is the mole ratio of HCl neutralized to H2O produced?

1: 2
2 : 1
1 : 1
2 : 2

A

2 : 1

57
Q

Fireworks often contain magnesium due to the bright light produced by burning this soft metal. This happens according to the following reaction:

2Mg + O2 –> 2MgO

How many moles of MgO will be produced if a firework that contains 0.456 mol of Mg explodes?

  1. 456 mol
  2. 912 mol
  3. 0188 mol
  4. 00810 mol
A

0.456 mol

58
Q

Fireworks often contain magnesium due to the bright light produced by burning this soft metal. This happens according to the following reaction:

2Mg + O2 \longrightarrow 2MgO

How many grams of O2 will be used if a firework that contains 0.456 mol of Mg explodes?

  1. 300 g
  2. 65 g
  3. 30 g
  4. 6 g
A

7.30 g

59
Q

The reaction between copper and silver nitrate produces beautiful silver flakes and a bright blue copper (II) nitrate solution according to the following reaction:

Cu + 2AgNO3 –> 2Ag + Cu(NO3)2

What is the ratio of moles of Cu metal required to moles of Ag produced by this reaction?

1: 2
2: 1
1: 1
2: 2

A

1:2

60
Q

The reaction between lead (II) nitrate and potassium iodide produces a bright yellow precipitate according to the following reaction:

Pb(NO3)2 + 2KI –> 2KNO3 + PbI2

How many moles of PbI2 will be produced if 0.321 moles of KI are entirely used during the reaction?

  1. 0803 mol
  2. 161 mol
  3. 321 mol
  4. 642 mol
A

0.161 mol

61
Q

The reaction between lead (II) nitrate and potassium iodide produces a bright yellow precipitate according to the following reaction:

Pb(NO3)2 + 2KI –> 2KNO3 + PbI2

How many grams of KNO3 will be produced if 0.321 moles of KI are entirely used during the reaction?

  1. 3 g
  2. 5 g
  3. 3 g
  4. 9 g
A

32.5 g

62
Q

The values and equation used in this problem will be used in questions 2 and 3 as well.

Lithium hydroxide is frequently used to neutralize sulfuric acid according to the equation:

2LiOH + H2SO4 –> 2H2O + Li2SO4.

If 5.6 g of LiOH reacts with 10.2 grams of H2SO4, LiOH is the limiting reactant.

True
False

A

False

63
Q

This is the same equation and amounts used in question 1. Use your work from problem 1 to assist you in problem 2.

Lithium hydroxide is frequently used to neutralize sulfuric acid according to the equation:

2LiOH + H2SO4 –> 2H2O + Li2SO4.

If 5.6 g of LiOH reacts with 10.2 grams of H2SO4, what is the theoretical yield of water in this reaction? (In other words, how much water do you expect to produce?)

4.2 g H2O
3.7 g H2O
13 g H2O
11 g H2O

A

3.7 g H2O

64
Q

This is the same equation and amounts used in questions 1 and 2. Use your work from problems 1 and 2 to assist you in problem 3.

Lithium hydroxide is frequently used to neutralize sulfuric acid according to the equation:

2LiOH + H2SO4 –> 2H2O + Li2SO4.

Marcus runs this reaction with 5.6 g of LiOH and 10.2 grams of H2SO4. What is the percent yield of this reaction if Marcus is able to produce 2.8 g of H2O?

55%
50.%
76%
130%

A

76%

65
Q

Use the following reaction to answer questions 4 and 5:

Potassium chloride reacts with lead (II) nitrate to form potassium nitrate and lead (II) chloride according to the following equation:

2KCl + Pb(NO3)2 –> 2KNO3 + PbCl2.

What is the limiting reactant if 24.9 g of KCl reacts with 20.4 grams of Pb(NO3)2?

KCl
Pb(NO3)2
KNO3
PbCl2

A

Pb(NO3)2

66
Q

This is the same information from question 4. Use your calculations from 4 to assist you.

Potassium chloride reacts with lead (II) nitrate to form potassium nitrate and lead (II) chloride according to the following equation:

2KCl + Pb(NO3)2 –> 2KNO3 + PbCl2.

Camryn runs this reaction with 24.9 g of KCl and 20.4 g of Pb(NO3)2 and produces 11.3 g of KNO3. What is the percent yield of this reaction?

91.1%
111%
82.3%
45.4%

A

91.1%

67
Q

Use the following information for questions 3 and 4.

Iron metal can be isolated by reaction iron (III) oxide and carbon monoxide to produce solid iron and carbon dioxide gas according to the equation :

Fe2O3 + 3CO –> 2Fe + 3CO2

If 12.5 grams of Fe2O3 reacts with 12.5 grams of CO, what is the limiting reactant?

Fe2O3
CO
Fe
CO2

A

Fe2O3

68
Q

Iron metal can be isolated by reaction iron (III) oxide and carbon monoxide to produce solid iron and carbon dioxide gas according to the equation :

Fe2O3 + 3CO –> 2Fe + 3CO2

When 12.5 grams of Fe2O3 reacts with 12.5 grams of CO, the reaction should produce 8.74 g of Fe. Cassie runs this reaction in her lab and is only able to produce 7.74g of Fe. What is her percent yield?

70.0%
88.6%
99.9%
113%

A

88.6%

69
Q

Use the following information to answer questions 5 and 6.

Zinc metal reacts very quickly with hydrochloric acid to produce zinc chloride and hydrogen gas according to the equation:

Zn + 2HCl –> ZnCl2 + H2

If 1.25 moles of Zn reacts with 3.00 moles of HCl, what is the theoretical yield of H2 for the reaction?

  1. 625 g
  2. 25 g
  3. 52 g
  4. 02 g
A

2.52 g

70
Q

Zinc metal reacts very quickly with hydrochloric acid to produce zinc chloride and hydrogen gas according to the equation:

Zn + 2HCl –> ZnCl2 + H2

If 1.25 moles of Zn reacts with 3.00 moles of HCl and produces 2.00 g of H2, what is the percent yield for this reaction?

  1. 4%
  2. 4%
  3. 3%
  4. 7%
A

79.4%

71
Q

Use the following information to answer questions 7, 8, and 9.

Silicon dioxide reacts with elemental carbon to produce silicon carbide and carbon monoxide gas according to the reaction:

SiO2 + 3C –> SiC + 2CO

If 2.25 moles of SiO2 react with 7.25 moles of C, what is the limiting reactant?

SiO2
C
SiC
CO

A

SiO2

72
Q

Silicon dioxide reacts with elemental carbon to produce silicon carbide and carbon monoxide gas according to the reaction:

SiO2 + 3C –> SiC + 2CO

If 2.25 moles of SiO2 react with 7.25 moles of C, what is the theoretical yield of SiC?

1.50 g SiC
135 g SiC
81.1 g SiC
90.2 g SiC

A

90.2 g SiC

73
Q

Silicon dioxide reacts with elemental carbon to produce silicon carbide and carbon monoxide gas according to the reaction:

SiO2 + 3C –> SiC + 2CO

If 2.25 moles of SiO2 react with 7.25 moles of C to produce 81.1 g of SiC in the lab, what is the percent yield for this reaction?

111%

  1. 9%
  2. 9%
  3. 0%
A

89.9%

74
Q

Mark is conducting a quantitative experiment combusting ethylene (C2H4), a highly flammable hydrocarbon, to produce carbon dioxide and water according to the following reaction:

C2H4 + 3O2 –> 2CO2 + 2H2O

Mark begins his experiment with 5.0 moles of ethylene which can theoretically produce 180 grams of water. He also has 5.0 moles of oxygen available which can theoretically produce 60. grams of water. At the end of his experiment, he has produced 55 grams of water.

Which of the following correctly identifies the limiting reactant and the percent yield for Mark’s experiment?

Limiting Reactant = Ethylene; Percent Yield = 31%
Limiting Reactant = Ethylene; Percent Yield = 92%
Limiting Reactant = Oxygen; Percent Yield = 31%
Limiting Reactant = Oxygen; Percent Yield = 92%

A

Limiting Reactant = Oxygen; Percent Yield = 92%

75
Q

Asphalt has a higher heat capacity than water.
True
False

A

False

76
Q

In a water molecule,
the oxygen end of the molecule is slightly positive and the hydrogen end is slightly negative.
the oxygen and hydrogen share the electrons equally.
the electrons spend more time with hydrogen than they spend with oxygen.
the oxygen end of the molecule is slightly negative and the hydrogen end is slightly positive.

A

the oxygen end of the molecule is slightly negative and the hydrogen end is slightly positive.

77
Q

The curved meniscus of water in a graduated cylinder can best be attributed to
water’s high heat capacity.
water’s densities of solid and liquid.
capillary action.
surface tension.

A

capillary action.

78
Q

Which of the following molecules can have hydrogen bonding intermolecular force

A. H2S

B. H3N

C. H3P

D. HBr

Answer A
Answer B
Answer C
Answer D

A

Answer B

79
Q 
The property of water that allows water molecules to stick to other substances is called
  cohesion. 
  adhesion. 
  density. 
  dissolving ability.
A

adhesion

80
Q 
If a substance is soluble in water, this means that it \_\_\_\_\_\_ in water.
  dissolves 
  decomposes 
  reacts 
  remains unchanged
A

dissolves

81
Q

Which of the following substances would be soluble in mineral oil?

A. H2O

B. HF

C. H3N

D. H2

Answer A
Answer B
Answer C
Answer D

A

Answer D

82
Q

When NaCl dissolves in water, what is attracted to the oxygen in water?
The chloride ion is attracted to the oxygen in water.
The sodium ion is attracted to the oxygen in water.
It is not attracted to water because it is nonpolar and water is polar.
NaCl has an overall positive charge and is attracted to the oxygen in water.

A

The sodium ion is attracted to the oxygen in water.

83
Q 
The attractive forces that keeps water molecules together and creates surface tension are called
  adhesive forces. 
  dispersion forces. 
  hydrogen bonding. 
  physical forces.
A

hydrogen bonding.

84
Q

From the solubility table, you would write Na2SO4 as Na2SO4 (s).
True
False

A

False

85
Q 
Which of the following states of matter increases solubility with increased temperature?
  Solid 
  Liquid 
  Gas 
  Plasma
A

Solid

86
Q 
When a substance can conduct electricity in water, it is called a(n) \_\_\_\_.
  nonelectrolyte 
  electrolyte 
  supersaturated 
  unsaturated
A

electrolyte

87
Q

If a solution is considered miscible, then the solute is a [ Select ] and the solvent is a [ Select ] .

A

liquid

liquid

88
Q 
If a solution has more solute dissolved in the solvent than the solvent can theoretically dissolve, then this solution is said to be
  saturated. 
  unsaturated. 
  supersaturated. 
  miscible.
A

supersaturated

89
Q

When potassium bromide is dissolved in water, which part is attracted to the oxygen in water?
Potassium bromide is nonpolar and therefore does not dissolve in water.
Potassium bromide is polar covalent and therefore does not break apart in water.
The potassium ion.
The chloride ion.

A

The potassium ion.

90
Q 
Which of the following states of matter increases solubility with decreased agitation?
  Solid. 
  Liquid 
  Gas 
  Plasma
A

Gas

91
Q

Which of the following compounds would be considered an electrolyte?

A. C6H12O6

B. NaOH

C. CO2

D. AgCl

Answer A
Answer B
Answer C
Answer D

A

Answer B

92
Q 
When oxygen gas is pumped into water to make a solution, oxygen is the
  solute. 
  solvent. 
  electrolyte. 
  solution.
A

solute

93
Q 
The reason granulated sugar dissolves quicker than a sugar cube is due to granulated sugars
  increased temperature 
  increased surface area 
  decreased surface area 
  increased heat capacity
A

increased surface area

94
Q 
What are the units of molarity?
  moles 
  grams/mole 
  moles/liter 
  grams/liter
A

moles/liter

95
Q

What concentration will a solution have if 0.286 moles of solid is added to 316 mL of water?

  1. 000905 M
  2. 905 M
  3. 000000905 M
  4. 10 M
A

0.905 M

96
Q

You want to make a concentration of 3.00 M KCl and you only have 71.2 g of KCl. How much water do you need to add to make the solution?

  1. 318 L
  2. 14 L
  3. 7 L
  4. 042 L
A

0.318 L

97
Q 
Which of the following does not change when you dilute a solution?
  Molarity of the solution 
  Volume of the solvent 
  Moles of the solute 
  Concentration of the solution
A

Moles of the solute

98
Q 
What final volume does a solution need to be diluted to if you start with 50 mL of a 10 M solution and you want a 4.8 M solution?
  24 mL 
  104 mL 
  54 mL 
  0.104 mL
A

104 mL

99
Q 
How much water must be added to 100 mL of a 12 M solution to make a 1.2 M solution?
  0.9 mL 
  1 mL 
  900 mL 
  1000 mL
A

900 mL

100
Q 
Which of the following does not change when a blue colored solution is diluted?
  The color of the solution. 
  The molarity of the solution. 
  The moles of solute. 
  The volume of solution.
A

The moles of solute.

101
Q

A concentrated solution is a solution where
more solute is dissolved a small amount of solvent.
less solute is dissolved in a small amount of solvent.
more solute is dissolved in a large amount of solvent.
less solute is dissolved in a large amount of solvent.

A

more solute is dissolved a small amount of solvent.

102
Q

Which of the following is not considered an example of a dilution?
Ice melting in a cup of sweet tea.
Water evaporating from a cup of chicken stock.
Adding water to bleach to use as a disinfectant.
Adding water to lemon juice to make lemonade.

A

Water evaporating from a cup of chicken stock.

103
Q 
How many grams of NaCl must be added to 100. mL of water to make a 0.550 M solution?
  55 grams 
  0.055 grams 
  0.094 grams 
  3.21 grams
A

3.21 grams

104
Q

What is the original concentration of a 0.335 L solution if water was added to the mixture to make 1.34 L of a 0.546 M solution?

  1. 18 M
  2. 0022 M
  3. 01 M
  4. 137 M
A

2.18 M

105
Q 
How much water needs to be added to 12 mL of a 5.1 M solution to make a 1.3 M solution?
  47 mL 
  0.047 mL 
  35 mL 
  0.035 mL
A

35 mL

106
Q 
When performing a dilution, the concentration of the final solution will always be \_\_\_\_ the original solution.
  higher than 
  lower than 
  equal to 
  unrelated to
A

lower than

107
Q 
What is the name of the following compound? H2S
  Sulfuric acid 
  Hydrosulfuric acid 
  Sulfurous acid 
  Dihydrogen sulfide
A

Hydrosulfuric acid

108
Q

What is the correct formula for nitrous acid?

A. HN

B. H3N

C. HNO3

D. HNO2

Answer A
Answer B
Answer C
Answer D

A

Answer D

109
Q 
A strong acid or base
  dissociates completely in water. 
  dissociates slightly in water. 
  does not dissociate in water. 
  does not mix with water.
A

dissociates completely in water.

110
Q

Which of the following is considered a strong base?

A. Mg(OH)2

B. Al(OH)3

C. Sr(OH)2

D. Ni(OH)2

Answer A
Answer B
Answer C
Answer D

A

Answer C

111
Q

In the following reaction, which one is the conjugate acid of the base?

H2O + NH3 –> OH- + NH4+

A. H2O

B. NH3

C. OH-

D. NH4+

Answer A
Answer B
Answer C
Answer D

A

Answer D

112
Q

What is the pH of a substance that has an [H+] = 1.27 · 10-6 M?

  1. 9
  2. 0
  3. 0
  4. 1
A

5.9

113
Q 
What are the products in a neutralization reaction?
  Water 
  Acid + base 
  Salt + water 
  Salt
A

Salt + water

114
Q

Which of the following reactions is a REDOX reaction?

A. H2S + 2NaOH –> 2H2O + Na2S

B. 6NaCl + Ca3P2 –> 2Na3P + 3CaCl2

C. C + O2 –> CO2

D. HCl + NaOH –> NaCl + H2O

Answer A
Answer B
Answer C
Answer D

A

Answer C

115
Q

In the following REDOX reaction, which atom is being oxidized?

2C2H6 + 7O2 –> 4CO2 + 6H2O

C
H
O
This is not a REDOX reaction.

A

C

116
Q

What type of reaction is the following reaction?

H2O + NH3 –> OH- + NH4+

REDOX reaction
Precipitation reaction
Oxidation reaction
Acid/base reaction

A

Acid/base reaction

117
Q

What type of reaction is the following reaction?

NaCl + AgNO3 –> NaNO3 + AgCl

REDOX reaction
Precipitation reaction
Oxidation reaction
Acid/base reaction

A

Precipitation reaction

118
Q 
When an atom is reduced, it
  gains electrons. 
  gains protons. 
  loses electrons. 
  loses protons.
A

gains electrons.

119
Q

Which of the following scenarios would be an acidic solution?

A. [H3O+] < [OH-]

B. [H3O+] = [OH-]

C. [H3O+] > [OH-]

D. [H3O+] is not related to [OH-]

Answer A
Answer B
Answer C
Answer D

A

Answer C

120
Q 
A solution has an [H+] = 4.58 · 10-9 M. This solution is
  acidic. 
  basic. 
  neutral. 
  oxidation.
A

basic.

121
Q

Which of the following is the correct chemical formula for chlorous acid?

A. HCl

B. HClO3

C. HClO2

D. HClO

Answer A
Answer B
Answer C
Answer D

A

Answer C

122
Q

______ is considered a weak acid because it _______ dissociates in water.

A. HF; completely

B. HNO3; slightly

C. H2SO4; completely

D. HClO; slightly

Answer A
Answer B
Answer C
Answer D

A

Answer D

123
Q

In the following reaction, which is considered a Bronsted-Lowry base?

H2O + F- –> HF + OH-

A. H2O

B. F-

C. HF

D. This is not an acid-base reaction

Answer A
Answer B
Answer C
Answer D

A

Answer B

124
Q

What type of reaction is the following reaction?

2 H2O2 LaTeX: –> 2 H2O + O2

REDOX reaction
Precipitation reaction
Neutralization reaction
Acid/base reaction

A

REDOX reaction

125
Q

Which of the following reactions is a neutralization reaction?

A. H2S + 2NaOH LaTeX: –> 2H2O + Na2S

B. 6NaCl + Ca3P2 LaTeX: –> 2Na3P + 3CaCl2

C. C + O2 LaTeX: –> CO2

D. 2HCl + Li2S LaTeX: –> 2LiCl + H2S

Answer A
Answer B
Answer C
Answer D

A

Answer A

126
Q

Which of the following shows an Arrhenius base?

A. NH3 + H+ LaTeX: –> NH4+

B. H2SO4 LaTeX: –> H+ + SO42-

C. NaOH LaTeX: –> Na+ + OH-

D. HCl LaTeX: –> H+ + Cl-

Answer A
Answer B
Answer C
Answer D

A

Answer C

127
Q

Which of the following reactions is a precipitation reaction?

A. HCl + NaOH LaTeX: –> H2O + NaCl

B. 3CaCl2 + 2(NH4)3PO4 LaTeX: –> Ca3(PO4)2 + 6NH4Cl

C. C + O2 LaTeX: –> CO2

D. 2Na + Cl2 LaTeX: –> 2NaCl

Answer A
Answer B
Answer C
Answer D

A

Answer B

128
Q 
What is the name for the compound, Mg(OH)2?
  Magnesium oxygen hydride 
  Magnesium dihydroxide 
  Magnesium oxygen dihydrogen 
  Magnesium hydroxide
A

Magnesium hydroxide

Chemistry (5 decks)

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