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Chemistry H > MODULE > Flashcards

MODULE Flashcards

1
Q

To separate ink dye you would use

A

chromatography

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2
Q

which piece of laboratory equipment would be the best to use to measure heat of reaction?

A

calorimeter

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3
Q

what is the molar mass of magnesium nitrate?

A

148.3 g/mole

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4
Q

what is the name of N2O5?

A

dinitrogen pentoxide

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5
Q

What is the volume of N2 at STP contains 3.0 x 10^21 molecules?

A

0.112 L

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6
Q

How many total ions are in 1.00 mole of Chromium (III) sulfate Cr2(SO4)3?

A

5 moles

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7
Q

What is the IUPAC name for PbO2?

A

Lead (IV) oxide

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8
Q

Which instrument is used to accurately measure the volume?
1. Pipette
2. Buret
3. Graduate Cylinder
4. Beaker
5. Erienmeyer flask

A

2 and 3

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9
Q

The product of 0.010 m x 0.0942 m would be written as

A

0.00094 m^2

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10
Q

Which is a homogeneous mixture?

A

salt water

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11
Q

What is the average atomic mass for an element with the abundance of isotopes shown?

Atomic mass, amu and percent abundances, %
62.93, 69.2
64.93, 30.8

A

63.5 amu

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12
Q

Which statement best describes the effect of raising temperature on the rate of a reaction?

A

it will increase because the molecules have a greater average kinetic energy.

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13
Q

Which gas molecules have the greatest average speed at STP?

A

NH3

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14
Q

Which process represent a physical change?

A

The condensation of steam

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15
Q

To increase the solubility of gases in liquids, one could

A

increase the pressure

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16
Q

which is the coefficient of oxygen in this equation when it is correctly balanced?

A

7

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17
Q

What is the volume of 18.99 g of fluorine, at the pressure of 1.00 atm and a temperature of 27 celsius?

A

12.30

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18
Q
A
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19
Q
A
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20
Q
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20
Q
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21
Q
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22
Q
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23
Q
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24
Q
A
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25
Q

How many hydrogen atoms are in 5.0 moles of hydrogen molecules?

A

6.02 x 10^24 atoms

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25
Q

The greenhouse effect is caused by

A

All of the above
(CH4, CO2, Chloroflourocarbons (CFC5)

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26
Q

If the molecular formula is C6H8O6, what is the empirical formula?

A

C3H4O3

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27
Q

A student determined the percentage of water in hydrated copper (II) sulfate. The results of three trials are 32.42%, 32.41%, 32.39%. The actual percentage of water is 26.08%. The results the students obtained were

A

precise but not accurate

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28
Q

How many total atoms are in 1.00 mole of calcium sulfate dehydrate CaSO4 2H2O?

A

12 moles

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29
Q

What is the sum of 3.36 m, 7.1 m and 2.358 m?

A

12.8 m

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30
Q

One liter of gas has a mass of 7.78 g at STP. What is the molar mass of this gas?

A

174.27 g

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31
Q

Which of the following is true for all the chemical reactions?

A

The total mass of products is equal to the total mass of reactants.

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32
Q

Which one of the molecules is most polar?

33
Q

What is the effect of a catalyst on the potential energy diagram?

A

decreasing in activation energy

33
Q

Two gas samples with the same volume at the temperature and pressure. They have the same

A

number of molecules

34
Q

What is the geometry around the middle carbon in the propene?

A

trigonal planar sp2 hybridization

35
Q

What H2O has a higher boiling point than H2S because

A

Hydrogen bonds are stronger in water

36
Q

Which of these is the correct number of protons (p+) and electron (e-) in the flouride ion, F-?

A

9 p+ and 10e-

37
Q

Calculate the amount of heat absorbed when 2.88 grams of CaO is produced according to their equation. CaCO3 (s) => CaO (s) + CO2 (g) DH = +176 KJ

38
Q

What is the total number of unpaired electrons in the ground state of an oxygen atom, O?

39
Q

The electron configuration 1s2 2s 2p6 3s2 3p6 is true for all of these except

40
Q

What is the heat of reaction for the endothermic reaction

41
Q

Which arrangement of elements demonstrates the trend for increasing atomic radius?

42
Q

Which series of elements represents increasing electronegativity?

43
Q

Which molecule contains polar bonds and is a polar molecule?

A

NH3
(Molecules shapes that will cancel polar bonds: trigonal planar, tetrahedron, linear, bipyramidal, octahedron)
(Molecular shapes that will not cancel polar bonds: bent, pyramidal)

44
Q

FeO3 (s) + 3CO (g) => 2 Fe (l) + 3CO2 (g)
Molar mass of Fe2O3 is 159.7 g.mole. What mass of Fe is formed from 1250 grams of Fe2O3?

45
Q

What do logs of wood burn slowly when in a pile, but rapidly when chopped into small pieces?

A

smaller pieces have a greater surface area in contact with the air.

46
Q

Which part of heating curve represents the boiling point for the substance?

A

D to E
(Temperature stays constant during phase change)

47
Q

In the energy diagram, what is the activation energy for the reversed reaction?

A

150 KJ (look at the graph provided)

47
Q

lithium, beryllium, sodium, and magnesium are neighbors on the period table. Which statement is true about four elements?

A

Lithium most resembles sodium in chemical properties

48
Q

Which set contains the least reactive elements?

A

Cu, Zn, Au

49
Q

Which substance is most soluble in water?

A

NaCl
(Polar molecules dissolve polar; non polar molecules dissolve non polar)

50
Q

Equal moles of each substance are spread on any icy road. Which would melt the most ice?

A

magnesium chloride, MgCl2
(dt = i Kf m)
(If it is molecular compound the number pf particles I is one.)
(If it is an ionic compound the number of particles I is the number of ions dissociated)

51
Q

What forces of attraction are present in graphite, diamond, and buckminsterfullerene (Bucky ball), which are all allotropes of carbon?

A

network covalent

52
Q

Al2(CO3)3 (s) + 6HCl (aq) => 2AlCl3 (aq) + 3H2O (l) + 3CO2 (g)
What volume of carbon dioxide gas CO2 would be produced at STP if 3.65 g of hydrochloric acid, Hal reacts with excess aluminum carbonate? Molar mass of Hal is 36.5 g/mole.

53
Q

A sample of methanol required 13.6 kJ of energy to be heated from 22.0 celsius to 37.0 celsius. How many grams of methanol were heated? Specific heat of methanol is 2.51 J.g C.

54
Q

Which pair of changes insures that a chemical system undergoes a spontaneous reaction?

A

a decrease in enthalpy and an increase in entropy
(dG less than 0 the reaction is spontaneous)
(dG = dH - TdS)

55
Q

If an isolated reaction has an equilibrium constant much smaller than 1, the reaction is

A

non spontaneous, favoring reactants
(Keq greater than 1 – product favored, spontaneous
Keq less than 1 – reactant favored, non spontaneous)

56
Q

In the reaction Ag (s) + 2H+ (aq) + NO2 (g) + H2O (l) the reducing agent is

A

Ag
(reducing agent = oxidized. Oxidation number increased)

57
Q

Given: N2 (g) + 3H2 (g) <–> 2Nh3 (g) + heat
When pressure is decreased, equilibrium shifts to the

A

reactants

(4 moles of gases react to form moles of gases. When pressure is decreased, equilibrium shifts to the side with more moles.)

58
Q

A water solution of which compound will turn blue litmus red?

A

NH4Cl
(look for a salt produced from the combination of strong acid and weak base)

59
Q

What change occurs during oxidation?

A

loss of electrons

60
Q

What particle is needed to compete this nuclear reaction>

A

4 2 He

Balance the mass number and atomic number

61
Q

How many milliliters of the 7.5 M H3PO4 stock solution should be added to distilled water to prepare 1.5 L of a 1.0 M solution?

62
Q

Which of the following mixtures is a colloid (cream like)?

63
Q

The pH of a solution with ][OH-] = 5.4 x 10 ^-6 M is

64
Q

How many moles of calcium hydroxide are needed to neutralize 2.0 moles of phosphoric acid?

A

3 moles
(titration) (not on the test)

65
Q

When an electron moves from a lower to a higher enevery level, the electron

A

absorbs a quantum of energy

66
Q

Based on the chemical reaction given, what is the most likely change in entropy?
CaCO3 (s) –> CaO (s) + CO2 (g)

67
Q

In which reaction is HSO3- (aq) acting as an acid?

A

HSO3- (aq) +NH3 (aq) –> SO3-2 (aq) +NH4+ (aq)

68
Q

Which of the following substances is less soluble in hot water than in cold water?

69
Q

Which of the following factors affect solubility?

A

Temperature and the nature of the solvent

70
Q

Which would be the resulting titration curve for the process if a weak base in a flask is titrated with a known concentration of a strong acid in a buret?

71
Q

Which of these would be the strongest acid with the largest Ka value?

A

HClO4
(Ka is stronger with addition of oxygen)

72
Q

What are the Bronsted-Lowry acids in the following equilibrium reaction?
CN = H2O <==> HCN +OH-

73
Q

What is one product of the reaction between KOH and Her?

74
Q

What is the oxidation states of Manganese, Mn in MnO4-?

75
Q

What is of the following is always true of the spontaneous reaction

A

It releases free energy

76
Q

What is the equilibrium constant expression for the reaction
CO2 (g) + C (s) <–> 2CO (g)

A

[CO]^2/[CO2]
(C (s) is not included in equilibrium expression)

77
Q

Calculate dH for the following reaction

C2H4 (g) + H2 (g) –> C2H6 (g)

(dHf for C2H4 (g) = 52.5 kJ/mol;
dHf for C2H6 (g) = -84.7 kJ.mol)

78
Q

What does the addition of a common ion do to the solubility of that ion?

A

decrease the solubility

79
Q

How many grams of sodium hydroxide NaOH should be added to 500 g of water to prepare a 0.10 m solution? Molar mass of NaOH is 40.0 g/mole

Chemistry H (11 decks)

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