HW 08
REVIEW QUESTIONS
Chapter 8
- Given the unbalanced equation shown below:
a) How many grams of
b) How many grams of NaCl are produced when 80.0 g of
2. Given the balanced equations below, how many moles of each reactant must react to produce 13.70 mole of
b) How many grams of NaCl are produced when 80.0 g of
2. Given the balanced equations below, how many moles of each reactant must react to produce 13.70 mole of
- What mass of
can be produced from the reaction of 25.0 g of with 75.0 g of according to the following equation:
- How many grams of
are produced when 152 g of react with 48.0 g of according to the following equation:
- When 50.0 g of
react completely with of are produced. What is the percent yield for this reaction? The unbalanced equation is given below:
- The reaction of calcium and nitrogen gas (shown below) can be carried out with
yield. In an experiment, 56.6 g of calcium are reacted with 30.5 g of nitrogen gas. What mass of calcium nitride is formed in this experiment?
- Hydrogen gas has been suggested as a clean fuel because it produces only water when it burns. If the reaction has a
yield, what mass of hydrogen gas would form 75.0 kg of water? - Diborane
can be produced by the unbalanced reaction shown below. If the reaction has an yield, how many grams of are needed to produce 20.0 g of diborane?
- Consider the reaction shown below:
a) Is this reaction endothermic or exothermic?
b) How much heat is released when 85.0 g of
10. Thermal decomposition of mercury (II) oxide occurs as shown below:
b) How much heat is released when 85.0 g of
10. Thermal decomposition of mercury (II) oxide occurs as shown below:
a) How much heat is needed to decompose 555 g of HgO ?
b) If 275 kJ of heat is absorbed, how many grams of mercury form?
11. Iron (II) sulfide reacts with HCl according to the reaction:
b) If 275 kJ of heat is absorbed, how many grams of mercury form?
11. Iron (II) sulfide reacts with HCl according to the reaction:
A reaction mixture initially contains 20.0 g of FeS and 23.8 g of HCl . When the reaction has occurred as completely as possible, what mass of which reactant is left?
12. People often use sodium bicarbonate as an antacid to neutralize excess hydrochloric acid in an upset stomach. (a) Write a balanced equation for the reaction of aqueous sodium bicarbonate and aqueous hydrochloric acid; (b) What mass of hydrochloric acid (in grams) can 2.5 g of sodium bicarbonate neutralize?
13. A solution contains an unknown mass of dissolved barium ions. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered, dried and found to have a mass of 258 mg . Based on this information, what mass of barium was in the original sample? (Assume that all of the barium was precipitated out of the solution by the reaction.)
14. Consider the reaction shown below:
12. People often use sodium bicarbonate as an antacid to neutralize excess hydrochloric acid in an upset stomach. (a) Write a balanced equation for the reaction of aqueous sodium bicarbonate and aqueous hydrochloric acid; (b) What mass of hydrochloric acid (in grams) can 2.5 g of sodium bicarbonate neutralize?
13. A solution contains an unknown mass of dissolved barium ions. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered, dried and found to have a mass of 258 mg . Based on this information, what mass of barium was in the original sample? (Assume that all of the barium was precipitated out of the solution by the reaction.)
14. Consider the reaction shown below:
A reaction flask initially contains 27.5 g of
15. Magnesium ions can be precipitated from seawater by addition of sodium hydroxide. How many grams of NaOH must be added to a sample of seawater to completely precipitate 88.4 mg of magnesium present? (Write a balanced equation for the reaction first.)
16. Pyrite (
15. Magnesium ions can be precipitated from seawater by addition of sodium hydroxide. How many grams of NaOH must be added to a sample of seawater to completely precipitate 88.4 mg of magnesium present? (Write a balanced equation for the reaction first.)
16. Pyrite (