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Chapter 13 > Chapter > Flashcards

Chapter Flashcards

1
Q

What do the coefficients in a chemical reaction specify?

A

The relative amounts in moles of each of the substances involved in the reaction

Coefficients indicate the ratio of reactants and products in a balanced chemical equation.

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2
Q

In the balanced equation 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O, how many molecules of CO2 are produced from 2 molecules of C8H18?

A

16 molecules of CO2

This reflects the stoichiometric ratio from the balanced equation.

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3
Q

What is the first step in balancing a chemical equation?

A

Write a skeletal equation by writing chemical formulas for each of the reactants and products

A skeletal equation serves as the starting point for balancing.

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4
Q

When balancing chemical equations, which ions should be balanced second?

A

Nonmetal ions (anions)

If a polyatomic anion exists on both sides, balance it as a unit.

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5
Q

Fill in the blank: The stoichiometric ratio acts as a ______ between the amount in moles of a reactant to moles of a product.

A

conversion factor

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6
Q

What is the stoichiometric ratio of C8H18 to CO2 in the combustion reaction?

A

2 moles C8H18 : 16 moles CO2

This ratio is derived from the balanced equation.

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7
Q

How many moles of CO2 are produced when 22.0 moles of C8H18 are combusted?

A

176 moles of CO2

Calculation based on the stoichiometric ratio.

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8
Q

What is the mass of CO2 produced when 3.6 × 10^15 grams of C8H18 is burned?

A

1.1 × 10^16 grams of CO2

This is determined through mole-to-mass conversion using stoichiometric ratios.

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9
Q

What should be done if the balanced equation contains coefficient fractions?

A

Clear these by multiplying the entire equation by the denominator of the fraction

This ensures whole number coefficients for clarity.

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10
Q

When balancing a chemical equation, which type of atoms should be balanced last?

A

Free elements

Always adjust the coefficient on the free element to balance.

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11
Q

True or False: In a balanced equation, the total number of each type of atom on both sides must be the same.

A

True

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12
Q

List the steps for balancing chemical equations.

A
  • Write a skeletal equation
  • Balance metal ions first
  • Balance nonmetal ions second
  • Balance free elements last
  • Clear coefficient fractions if necessary
  • Check the balance

Following these steps ensures a systematic approach to balancing equations.

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13
Q

What is the balanced equation for the combustion of butane (C4H10) with oxygen?

A

C4H10 + O2 → CO2 + H2O

This skeletal equation needs to be balanced through the steps outlined.

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14
Q

What is the balanced equation for the combustion of butane (C4H10)?

A

C4H10(g) + 5 O2(g) → 4 CO2(g) + 5 H2O(g)

This equation shows butane reacting with oxygen to produce carbon dioxide and water.

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15
Q

What defines a chemical change?

A

Changes that alter the composition of matter

During a chemical change, atoms rearrange to form new substances.

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16
Q

Give an example of a chemical change.

A

Rusting of iron

Rust occurs when iron reacts with oxygen, forming iron(III) oxide (Fe2O3).

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17
Q

What is a physical change?

A

Changes that alter only the state or appearance without changing composition

Example: Water boiling to become steam.

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18
Q

What is the average rise in atmospheric temperature since 1860?

A

0.8 °C (1.4 °F)

This temperature change coincides with a 37% rise in atmospheric CO2 levels.

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19
Q

What are greenhouse gases?

A

Gases that allow sunlight in, warm the Earth’s surface, and prevent heat from escaping

They play a crucial role in the greenhouse effect.

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20
Q

What is stoichiometry?

A

The study of the numerical relationship between chemical quantities in a chemical reaction

It involves balancing chemical equations and calculating reactants and products.

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21
Q

What is a limiting reactant?

A

The reactant that is completely consumed in a reaction

It determines the maximum amount of product that can be formed.

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22
Q

What is the theoretical yield?

A

The maximum amount of product that can be formed from the limiting reactant

It is calculated based on stoichiometry.

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23
Q

What is a physical change?

A

Changes that alter only the state or appearance, but not the composition

The identity of the substance remains the same.

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24
Q

Fill in the blank: A _____ change results in a new substance being formed.

A

chemical

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25
Q

Fill in the blank: In reactions involving multiple reactants, the reactant that limits the amount of product is called the _____ reactant.

A

limiting

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26
Q

True or False: The balance between incoming and outgoing energy from the sun determines Earth’s average temperature.

A

True

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27
Q

What are the states of matter indicated in chemical equations?

A

Gas (g), liquid (l), solid (s), aqueous (aq)

These states describe the physical form of reactants and products.

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28
Q

What is the first step in balancing chemical equations?

A

Write a skeletal (unbalanced) equation

This involves writing chemical formulas for each of the reactants and products.

29
Q

What happens if the balanced equation contains coefficient fractions?

A

Multiply the entire equation by the denominator of the fraction

This clears the fractions and helps in balancing.

30
Q

What is the importance of confirming that a chemical equation is balanced?

A

To ensure the law of conservation of mass is upheld

The number of atoms of each element must be the same on both sides of the equation.

31
Q

What is the role of halogens in chemical reactions?

A

They form 1- anions and react with metals to create ionic compounds

Example: Halogens react with hydrogen to produce hydrogen halides.

32
Q

What is the relationship between moles of carbon dioxide and glucose in photosynthesis?

A

1 mole of glucose is produced from 6 moles of carbon dioxide

The balanced equation for photosynthesis is 6 CO2(g) + 6 H2O(l) → 6 O2(g) + C6H12O6(aq).

33
Q

Fill in the blank: The reactant in excess is any reactant that occurs in a quantity greater than is required to completely react with the _____ reactant.

A

limiting

34
Q

What does the term ‘percent yield’ refer to?

A

The ratio of the actual yield to the theoretical yield, expressed as a percentage

It indicates the efficiency of a reaction.

35
Q

What is the molar mass of carbon (C)?

A

12.01 g/mol

36
Q

What is the molar mass of titanium dioxide (TiO2)?

A

79.87 g/mol

37
Q

In the reaction of Fe2O3 and CO, which reactant is the limiting reactant?

A

CO

38
Q

What is the balanced equation for the reaction of potassium and bromine?

A

2 K(s) + Br2(g) → 2 KBr(s)

39
Q

What products are formed when alkali metals react with water?

A
  • Dissolved alkali metal ion
  • Hydroxide ion
  • Hydrogen gas
40
Q

What is a combustion reaction?

A

A reaction involving a substance reacting with O2 to form oxygen-containing compounds.

41
Q

What is produced in the combustion of methane?

A
  • CO2(g)
  • H2O(g)
  • Heat
42
Q

What is the molar mass of carbon dioxide (CO2)?

A

44.01 g/mol

43
Q

What is the theoretical yield of ammonia (NH3) when NO is the limiting reactant?

A

49.0 g

44
Q

What is the balanced equation for the formation of sulfuric acid (H2SO4) from sulfur dioxide (SO2)?

A

2 SO2(g) + O2(g) + 2 H2O(l) → 2 H2SO4(aq)

45
Q

What is the molar mass of sulfuric acid (H2SO4)?

A

98.09 g/mol

46
Q

What is the limiting reactant in the reaction of titanium dioxide (TiO2) and carbon (C) if 28.6 kg C reacts with 88.2 kg TiO2?

A

To be determined based on stoichiometric calculations

47
Q

What is the percent yield if 42.8 kg of titanium is produced from the reaction of TiO2 and C?

A

To be calculated based on theoretical yield vs actual yield

48
Q

Fill in the blank: The reaction of alkali metals with halogens typically forms ______.

A

[metal halide]

49
Q

True or False: The reaction of alkali metals with water is typically non-exothermic.

A

False

50
Q

What is the balanced equation for the complete combustion of methanol (CH3OH)?

A

2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g)

51
Q

What is the main product of the combustion of organic substances?

A

CO2 and H2O

52
Q

What are the products of the reaction between nitrogen gas (N2) and hydrogen gas (H2) to form ammonia (NH3)?

A

2 NH3(g)

53
Q

In stoichiometry, what is the first step when given a mass of a reactant?

A

Convert mass to moles using molar mass.

54
Q

What is the relationship used to convert from grams of SO2 to grams of H2SO4?

A

2 mol SO2 : 2 mol H2SO4 from the balanced equation

55
Q

How many pizzas can be made if you have enough crusts for 4, cheese for 5, but only enough tomato sauce for 3?

A

3 pizzas

56
Q

What is the limiting reactant in a chemical reaction?

A

The reactant that is completely consumed and limits the amount of product.

57
Q

In the pizza analogy, which ingredient is the limiting reactant?

A

Tomato sauce

58
Q

What is the actual yield in a chemical reaction?

A

The amount of product actually produced.

59
Q

What is the theoretical yield in a chemical reaction?

A

The amount of product that can be made based on the limiting reactant.

60
Q

How is percent yield calculated?

A

Percent yield = (actual yield / theoretical yield) x 100

61
Q

Fill in the blank: The maximum number of pizzas that can be made depends on the _______.

A

[limiting reactant]

62
Q

What are the molar masses of NO and H2?

A

NO = 30.01 g/mol; H2 = 2.02 g/mol

63
Q

What does the term ‘reactant in excess’ refer to?

A

Any reactant that occurs in a quantity greater than required to completely react with the limiting reactant.

64
Q

True or False: The theoretical yield is always equal to the actual yield.

A

False

65
Q

What is the significance of the limiting reactant in stoichiometry?

A

It determines the maximum amount of product that can be formed.

66
Q

What is the relationship between moles and grams in stoichiometry?

A

Moles can be converted to grams using molar mass.

67
Q

Fill in the blank: The reactant that makes the least amount of product is called the _______.

A

[limiting reactant]

68
Q

What is the role of stoichiometric relationships in determining theoretical yield?

A

They convert between moles of reactant and moles of product.

Chapter 13 (3 decks)

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