Chemistry Chapter 10

when hydrogen sulfide reacts with oxygen, water and sulfur dioxide are produced. The balanced equation for this reaction is 2H2S + 3O2 --> 2H2O + 2SO2. for all parts of this question, consider what will happen if 1.254 moles of hydrogen sulfide react. - how many moles of oxygen are consumed? - how many moles of water are produced? - how many moles are sulfur dioxide are produced?

- 1.881 molO2 - 1.254 mol H2O - 1.254 mol SO2

an experimenter recovers 0.5210 g of sodium sulfate from the neutralization of sodium hydroxide by sulfuric acid. How many grams of sulfuric acid reacted?

0.2598 g H2SO4

What mass in grams of hydrogen has to react to transfer 71.90 kJ of energy from the reaction 2 H2 (g) + O2 (g) 2 H2O (g) + 484 kJ?

0.6002g H2

Nitrogen monoxide is produced by combustion in an automobile engine. It can then react with oxygen: 2 NO + O2 2 NO2. If 5.74 g of oxygen gas reacts with excess nitrogen monoxide in a system in which the percentage yield of nitrogen dioxide is 80.2 %, what is the actual yield of nitrogen dioxide?

13.2 gNO2

in our bodies, sugar is broken down by reacting with oxygen to produce water and carbon dioxide. how many moles of carbon dioxide will be formed upon the complete reaction of 0.42 moles of glucose (C6H12O6) with excess oxygen gas?

2.5 mol CO2

H = -75.8 kJ for the reaction S (s) + 2 CO (g) SO2 (g) + 2 C (s). When 10.1 g of sulfur reacts with excess carbon monoxide, what quantity of energy, expressed in kilojoules, is transferred?

23.9 kj is released

hydrogen iodide is a colorless, nonflammable, and corrosive gas with a penetrating and suffocating odor. It can be prepared by direct reaction of its elements: H2 + I2 --> 2HI. It is desired to produce 331 g of hydrogen iodide in a process in which the percentage yield is 71.1%. How many grams of hydrogen gas will need to be reacted?

3.68g H2

Carbon dioxide can be removed from the air by reaction with potassium hydroxide: CO2 + 2 KOH K2CO3 + H2O. If 15 g of carbon dioxide reacts with 43 g of potassium hydroxide, what mass of potassium carbonate will be formed?

47g K2CO3

Carborundum, SiC, is widely used as an abrasive in industrial grinding wheels. It is prepared by the reaction of sand, SiO2, with the carbon in coke: SiO2 + 3 C SiC + 2 CO . What mass in kilograms of carborundum can be prepared from 727 kg of coke that is 88.9% carbon?

719 kg SiC

Nitroglycerine is the explosive ingredient in industrial dynamite. Much of its destructive force comes from the sudden creation of large volumes of gaseous products. A great deal of energy is transferred, too. H = -6.17 x 103 kJ for the equation 4 C3H5(NO3)3 (l) 12 CO2 (g) + 10 H2O (g) + 6 N2 + O2. Calculate the weight in grams of nitroglycerine that must be used in a blasting operation that requires 5.88 x 104 kJ of energy.

8.66 x 10^3 g C3H5(NO3)3

Butane gas is used as fuel for camp stoves, producing heat in the reaction given below. When 4.14 g of butane reacts with excess oxygen gas, the reaction yields 11.0 g of carbon dioxide. what is the percentage yield in this reaction? 2C4H10 + 13O2 --> 8CO2 + 10H2O

88.0%

Butane, C4H10, is a common fuel used for heating homes in areas not served by natural gas. The equation for its combustion is 2C4H10 + 13O2 --> 8CO2 + 10H2O. All parts of this question are related to this reaction. - how many grams of butane can be burned by 2.54 moles of oxygen? - if 7.789g of oxygen is used in burning butane, how many moles of water result? - calculate the number of grams of carbon dioxide that will be produced by burning 1.25 g of butane. - how many grams of oxygen are used in a reaction that produces 0.915 g of water?

- 22.7g C4H10 - 0.1872 mol H2O - 3.78 g CO2 - 2.11 g O2

trinitrotoluene is the chemical name for the explosive commonly known as TNT. Its formula is C7H5N3O6. TNT is manufactured by the reaction of toluene, C7H8, with nitric acid: C7H8 + 3 HNO3 --> C7H5N3O6 + 3H2O - how much nitric acid is needed to react completely with 1.90 kg of toluene? - how many kilograms of TNT can be produced in the reaction?

- 3.90 kg HNO3 - 4.68 kg TNT

Sodium carbonate can neutralize nitric acid by the reaction 2 HNO3 + Na2CO3 2 NaNO3 + H2O + CO2. - Is 135 g of sodium carbonate enough to neutralize a solution that contains 188 g of nitric acid? - How many grams of carbon dioxide will be released in the reaction?

- No. 188g HNO3 requires 158 g of Na2CO3. - 56.1g CO2

actual yield

measured amount of product isolated from the reaction

percentage yield

the actual yield of a chemical reaction expressed as a percentage of theoretical yield.

Ideal yield

the amount of product formed from the complete conversion of the given amount of reactant to product.

limiting reactant

the reactant first totally consumed in a reaction, thereby determining the maximum yield possible.

excess reactant

the reactant(s) in a chemical reaction that remain when the reaction is complete.