Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation:

2Al(s) + 2NaOH(aq) + 6H2O(l)------> 2NaAl(OH)4(aq) + 3H2(g)

The product gas, H2, is collected over water at a temperature of 20 C and a pressure of 757.0 mm Hg. If the wet gas formed occupies a volume of 9.96 L, the number of grams of H2 formed is = g. The vapor pressure of water is 17.5 mm Hg at 20 C.

What volume of oxygen gas is produced when 52.2 g of mercury(II) oxide reacts completely according to the following reaction at 25 C and 1 atm?

mercury(II) oxide(s)----> mercury(l) + oxygen(g)

Volume = L

What volume of butane (C4H10) is required to produce 102 liters of water according to the following reaction? (All gases are at the same temperature and pressure.)

butane (C4H10) (g) + oxygen(g)-----> carbon dioxide(g) + water(g)

Volume = L

A mixture of carbon dioxide and nitrogen gases at a total pressure of 927 mm Hg contains carbon dioxide at a partial pressure of 271 mm Hg. If the gas mixture contains 3.94 grams of carbon dioxide, how many grams of nitrogen are present?

Mass = g N2

A mixture of argon and carbon dioxide gases contains argon at a partial pressure of 202 mm Hg and carbon dioxide at a partial pressure of 494 mm Hg. What is the mole fraction of each gas in the mixture?

X_Ar = X_CO2 =