1. a. Sulfur in gasoline can produce sulfuric acid, H2SO4, according to the two-step process shown below. For each 125 g
of sulfur in gasoline, how many moles of H2SO4 will be produced?
b. What i
s the total volume of oxygen consumed by the
combustion of 125 g of sulfur at 27oC and 100. kPa?
2. a. Write an equation for the reaction between hydrochloric acid and calcium carbonate.
b. Determine the volume of 1.50 mol dm–3 hydrochloric acid that would react with exactly 1.25 g of calcium
carbonate.
c. Calculate the volume of carbon dioxide, measured at 273 K and
1.01×105 Pa, which would be produced when 1.25 g of calcium carbonate reacts completely with the
hydrochloric acid.
3. A toxic gas, A, consists of 53.8% nitrogen and 46.2% carbon by mass. At 273 K and
1.01×105 Pa, 1.048 g of A occupies 462 cm3. Determine the empirical formula of A.
Calculate the molar mass of the compound and determine its molecular structure.
4. Hydrogen gas can be obtained by placing an active metal in an acid. Zinc when placed in hydrochloric acid will
bubble giving off a gas. That gas is hydrogen leaving a solution of aqueous zinc chloride.
a. With an excess of hydrochloric acid, would you attain more hydrogen gas from zinc or silver?
b. If the reaction yield is 70.2%, what volume of 1.25 M HCl would be needed to product 1.00 L of hydrogen gas at
101.3 kPa and 24.0 oC?
c. What is the minimum mass of zinc that could be used in “b” in a reaction if 70.2% yield?
5. At 800-1200 oC, water will react with methane gas to produce carbon monoxide gas and hydrogen gas.
In a second reaction the carbon monoxide will reacted with water at 360 oC to produce carbon dioxide and hydrogen.
a. Write the two reaction equations indicating conditions and states of matter.
b. If a reaction begins with 200.0 kg of methane and 200.0 kg of water, what maximum mass of hydrogen can be
produced in the 1st reaction?
c. What mass of which compound is left over at the end of reaction 1
d. If the 1st reaction has 63.5% yield and the 2nd reaction a 95.5% yield; what is the minimum mass of methane and
or water needed to produce 1.00 L hydrogen gas cooled to 32 oF and at 14.7 psi?
6. 5.005 grams of alcohol were completely burned in the air. 10.99 g of carbon dioxide and 6.002 g of water
were recovered. What is the empirical and molecular formula of alcohol?