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Chemistry > Chapter 9 > Flashcards

Chapter 9 Flashcards

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1
Q

The reactant that limits the amount of the other reactant that can combine and the amount of product that can form in a chemical reaction.

A

Limiting Reactant

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2
Q

The volume occupied by one mole of a gas at STP.

A

Standard molar volume

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2
Q

Use the balanced chemical equation below to calculate the number of moles of carbon needed to react completely with 135 grams of iron(III) oxide.

2Fe2O3 + 3C –> 4Fe +3CO2

A

Use the molar mass of the first substance to convert to moles, then use the mole ratio from the coefficients to convert to moles of the other substance.

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3
Q

Using the balanced equation below, calculate the number of moles of hydrogen needed to react completely with 2.5 moles of nitrogen.

3H2 + N2 –> 2NH3

A

Use the mole ratio from the coefficients to convert from moles of one substance to moles of another substance.

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4
Q

Use the balanced reaction below to calculate the theoretical yield of tin(II) fluoride from 119g of tin and 43.0g of hydrogen fluoride. What is the limiting reactant?

Sn + 2HF –> SnF2 + H2

If the actual yield is 149g, what is the percent yield?

A

The smaller answer is the theoretical yield. The reactant that limits the amount of product is the limiting reactant.

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7
Q

Fill in each circle:

A
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8
Q

What volume would 0.68mol of ozone gas occupy at STP?

A

1 mole of any gas at STP occupies 22.4 liters at STP.

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9
Q

Using the balanced equation below, what mass of sodium peroxide would be needed to react completely with 5.0L of CO2, at STP?

2Na2O2(s) + 2CO2(g) –> 2Na2CO3(s) + O2(g)

A

Since at STP, use the standard molar volume to convert liters to moles. Then use the mole ratio from the coefficients to convert to moles of the second substance. Finally, use the molar mass of the second substance to convert to grams.

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10
Q

The values of standard temperature and standard temperature, respectively

A

0°C and 1 atmosphere

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11
Q

Fill in the information missing beside each line.

A
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11
Q

The substance that is not used up completely in a chemical reaction.

A

Excess Reactant

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11
Q

The maximum amount of product that can be produced from a given amount of reactant.

A

Theoretical yield

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11
Q

Use the balanced chemical equation below to calculate the mass in grams of sodium hypochlorite that could be produced from 0.50mol of NaOH, assuming an excess of chlorine:

2NaOH + Cl2 –> NaClO + NaCl + H2O

A

Convert from moles of the first substance to moles of the second substance using the mole ratio from the coefficients, then use the molar mass of the second substance to convert to grams.

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12
Q

A conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction.

A

Mole Ratio

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13
Q

Use the balanced chemical equation below to calculate the mass in grams of chlorine needed to produce 17g of sodium chloride, assuming an excess of sodium hydroxide:

2NaOH + Cl2 –> NaClO + NaCl + H2O

A

Convert the mass of the first substance to moles using its molar mass. Then, convert from moles of the first substance to moles of the second substance using the mole ratio from the coefficients. Finally, convert to mass of the second substance using its molar mass.

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14
Q

Use the reaction below to calculate the volume of N2O in liters that could be produced from 24g of ammonium nitrate at STP

NH4NO3(s) –> N2O(g) + 2H2O(g)

A
15
Q

Using the balanced equation below, how many milliliters of oxygen would be produced from 84mL of carbon dioxide and an excess of of sodium perioxide, assuming the gases are at the same temperature and pressure?

2Na2O2(s) + 2CO2(g) –> 2Na2CO3(s) + O2(g)

A

At equal temperature and pressure, the coefficients from the balanced equation can be interpreted to mean volumes of gases.

18
Q

The meaning of the abbreviation STP is

A

Standard temperature and pressure

19
Q

Use the balanced chemical equation below to calculate the number of moles of sodium hydroxide needed to react completely with 30.0g of Cl2:

2NaOH + Cl2 –> NaClO + NaCl + H2O

A

Use the molar mass of the first substance to convert to moles, then use the mole ratio from the coefficients to convert to moles of the other substance.

21
Q

The ratio of the actual yield to the theoretical yield, multiplied by 100

A

Percentage yield

22
Q

What volume would 3.42 moles of xenon gas occupy at STP?

A

1 mole of any gas occupies 22.4 liters at STP.

23
Q

Use the balanced chemical equation below to calculate the mass in grams of iron that could be produced from 8.43g of iron(III) oxide, assuming an excess of carbon.

2Fe2O3 + 3C –> 4Fe +3CO2

A

Convert the mass of the first substance to moles using its molar mass. Then, convert from moles of the first substance to moles of the second substance using the mole ratio from the coefficients. Finally, convert to mass of the second substance using its molar mass.

23
Q

If 24g of iron(III) oxide reacts with 3.1g of carbon, what is the theoretical yield of iron? What is the limiting reactant?

2Fe2O3 + 3C –> 4Fe +3CO2

If the actual yield is 14g, what is the percent yield?

A

The smaller answer is the theoretical yield. The reactant that limits the amount of product is the limiting reactant.

24
Q

At STP, one mole of any gas occupied a volume of…

A

22.4L

25
Q

Use the balanced chemical equation below to calculate the mass in grams of iron that could be produced from 12 moles of carbon, assuming an excess of iron(III) oxide.

2Fe2O3 + 3C –> 4Fe +3CO2

A

Convert from moles of the first substance to moles of the second substance using the mole ratio from the coefficients, then use the molar mass of the second substance to convert to grams.

26
Q

Use the balanced chemical equation below to calculate the number of moles of carbon dioxide produced if 4.5 moles of iron(III) oxide react with an excess of carbon.

2Fe2O3 + 3C –> 4Fe +3CO2

A

Use the mole ratio from the coefficients to convert from moles of one substance to moles of another substance.

27
Q

How many moles of helium would be contained in a 12L sample at STP?

A

One mole of any gas occupies 22.4 liters at STP.

28
Q

Use the reaction below to calculate the number of liters of N2O gas produced if 5.0L of water vapor is also produced at the same temperature and pressure?

NH4NO3(s) –> N2O(g) + 2H2O(g)

A

The coefficients from a balanced equation can be used to relate volumes of gases at the same temperature and pressure.

29
Q

How many moles of cabon dioxide would be contained in a 54L sample at STP?

A

One mole of any gas occupies 22.4 liters at STP

30
Q

Involves the mass relationships between reactants and products in a chemical reaction.

A

Reaction Stoichiometry

31
Q

The measured amount of product obtained from a reaction.

A

Actual yield

Chemistry (13 decks)

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