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Elements Quiz > Chemistry Chapter 7-8 > Flashcards

Chemistry Chapter 7-8 Flashcards

1
Q

Combination

A

A+B = AB

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2
Q

Decomposition

A

AB = A+B

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3
Q

Single Replacement

A

A+BC = AC+B

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4
Q

Double Replacement

A

AB+CD = AD+CB

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5
Q

Combustion

A

Cx + Hy + O2 = CO2 + H2O

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6
Q

Steps of Combustion

A

Step 1: Put 2 in front of CxHy and distribute
Step 2: Go to H and H2O, balance and distribute
Step 3: Balance C in CO2 and distribute
Step 4: Add up Os on the right and the balance on the left
Step 5: Reduce if everything is reducable
Add Ratio and Balanced

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7
Q

OIL RIG

A

Oxidation is loss of electrons
Reduction is gain of electrons

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8
Q

Rules of Oxidation Reduction

A

1: Assign free elements a charge of 0
Ex: Cu or Fe2
Diatomic elements are free elements
2: Assign other charges based on oxidation numbers charges
ex: 2Cu^0 + O2^0 = 2Cu^+2O-2
3: Compare the charges and identify as oxidation or reduction

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9
Q

Oxidation reaction is when

A

0 goes to positive charge
Loses electrons
ex: 0 to 2+

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10
Q

Reduction reaction is when

A

0 goes to negative charge
Gains electrons
ex: 0 to 2-

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11
Q

If there is an e- on the left it is

A

reduction

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12
Q

If there is an e- on the right it is

A

oxidation

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13
Q

Oxidation always

A

loses electrons, may also be seen as an addition of oxygen or loss of hydrogen

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14
Q

Reduction always

A

gains electrons, may also be seen as loss of oxygen or gain of hydrogen

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15
Q

Half Redox reaction

A

Cu^0 + 2AgNO3 = Cu(NO3)2 + 2Ag
Cu goes from 0 to 2+
Ag goes from 1+ to 0

Half Redox:
Cu^0 = Cu^+2 + 2e-
Oxidation

Ag^+1 + e- = Ag^0
Reduction

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16
Q

What is a mole?

A

Unit of measurement, amount of a pure substance containing the same number of chemical units (atoms or molecules)

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17
Q

Avagadro’s Number

A

6.02 x 10^23 particles

1 mole / 6.02 x 10^23 or 6.02 x 10^23 / 1 mole

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18
Q

Moles of an element in a compound

A

Subscripts are used to write conversion factors for moles of an element

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19
Q

How many atoms of O are in 0.150 mole of C9H8O4?

A

3.61 x 10^23 atoms of O

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20
Q

How many CO2 molecules are in 0.500 mole of CO2?

A

3.01 x 10^23 molecules of CO2

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21
Q

What is the number of moles in 1.8 x 10^24 atoms of S?

A

3.0 moles of S

22
Q

Molar Mass

A

quantity in grams that equals atomic mass
ex: Na molar mass = 23g
H2 molar mass = 2g

23
Q

Molar mass of compounds

A

Add all element’s molar mass together
ex: C2H6O
C = 2 x 12.01
H = 6 x 1.01
O = 1 x 16.0
= 46.0 g/mol

24
Q

Calculations using molar mass

A

A box of salt contains 737g of NaCl, how many moles of NaCl are in the box?
12.6 moles of NaCl

25
Q

Law of conservation of mass

A

Matter cannot be created or destroyed
No change in total mass occurs
Mass of products is equal to mass of reactants

26
Q

Mole-Mole Factors, how many moles of each reactant and product are in 2Fe + 3S = Fe^2S^3

A

2 moles Fe, 3 moles S, 1 mole Fe2S3

27
Q

What is the mole mole factor for 3H2 + N2 = 2NH3

A

1 mole N2 / 3 mole H2 or 3 mole H2 / 1 mole N2

28
Q

Calculations using mole factors

A

4Fe + 3O2 = 2Fe2O3
How many moles of Fe2O3 can form from 6.0 moles of O3?
4.0 mole of Fe2O3

29
Q

How many mole of Fe are needed for the reaction of 12.0 mole of O2?
4Fe + 3O2 = 2Fe2O3

A

16.0 mole of Fe

30
Q

Converting mass calculations (g to mole to g)

A

Multiply the top first, then the divide by the bottom

4Na + O2 = 2Na2O
How many grams of Na2O are produced when 57.5 grams of Na react?
77.5 g NaO2

31
Q

Limiting Reactant (LR)

A

Substance that is used up first
Limits the amount of product that can form
Reactant that runs out first

32
Q

Excess reactant

A

What doesn’t run out/what is left over

33
Q

Calculating LR

A

Ex: You have 3 mole of CO and 5 mole of H2, how many mole of CH4O?
CO + 2H2 = CH4O

H2 is the LR

34
Q

What is the LR in this equation

A

N2 + 3H2 = 2NH3
You have 2.50 g N2 and 2.00 g H2, what is the LR of 2NH3?

N2 is the LR

35
Q

Exothermic

A

Heat is released, negative #
ex: H2 + Cl2 = 2HCl + 185 kj
Heat = -185

36
Q

Endothermic

A

Heat is absorbed, positive #
ex: N2 + O2 + 180 kj = 2NO
Heat = 180 kj

37
Q

Heat of reaction is

A

-the amount absorbed or released during a reaction that takes place at constant pressure
-Change occurs when reactants interact, bonds break apart or when products form

38
Q

Heat of reaction formula

A

Heat = H (products) - H (reactants)

39
Q

How much heat in Kj is released when nitrogen and hydrogen react to form 50.0 g of ammonia?
Heat = -92.2 Kj

A

N2 + 3H2 = 2NH3
- 135 Kj
Exothermic

40
Q

Combined Gas Law formula

A

P1V1/T1 = P2V2/T2

41
Q

Boyle’s Law

A

T and n are constant
P1V1 = P2V2

42
Q

Charle’s Law

A

P and n are constant
V1/T1 = V2/T2

43
Q

Gay - Lussac’s Law

A

V and n are constant
P1/T1 = P2/T2

44
Q

In combined gas laws, what is always constant?

A

n = moles
Temp always needs to be in Kelvin

45
Q

Dalton’s law of partial pressure

A

P total = P1 + P2
Rearrange to solve for unknown

46
Q

Ideal Gas Law

A

Pv = nRT
P = pressure
v = volume
n = moles
R = gas law constant
T = temp

47
Q

How many L in 1 mole?

A

1 mole = 22.4 L

48
Q

Standard pressure

A

1 atm

49
Q

How many mmHg is in 1 atm

A

760 mmHg

50
Q

How many kpa is in 1 atm

A

101.3 kpa

51
Q

Absolute zero =

A

0 Kelvin or -273 C

52
Q
A

Elements Quiz (3 decks)

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