Daily Problem #15 1. A mixture of gases contains 0.31 mol CH, 0.25 mol C2Ho, and
ID: 547312 • Letter: D
Question
Daily Problem #15 1. A mixture of gases contains 0.31 mol CH, 0.25 mol C2Ho, and 0.29 mol CsHs. The total pressure is 1.50 atm. Calculate the partial pressures of the gases. A piece of sodium metal reacts completely with water as follows: 2. 2Nas) + 2 1601) 2 NaOHao + Hag) The hydrogen gas generated is collected over water at 25.0°C·The volume of the gas is 246 mL measured at 1.00 atm. Calculate the number of grams of sodium used in the reaction. (Vapor pressure of water at 25°C 23.8 mmHg) 3. Some commercial drain cleaners contain a mixture of sodium hydroxide and aluminum powder. occurs: When the mixture is poured down a clogged drain, the following reaction The heat generated in this reaction helps melt away obstructions such as grease, and the hydrogen gas released stirs up the solids clogging the drain. Calculate the volume of H2 formed at 23°C and 1.00 atm if 3.12 g of Al are treated with an excess of NaOH.Explanation / Answer
Q1
Partial pressure of any gas is given by
P-i = x-i * Ptotal
x-i = mol of i / Total mol
then
P-i = mol of i / Total mol * Ptotal
total mol = 0.31+0.25 + 0.29 = 0.85
P-CH4 = 0.31 / (0.85) * 1.5 = 0.547 atm
P-C2H6 = 0.25 / (0.85) * 1.5 = 0.441 atm
P-CH4 = 0.29/ (0.85) * 1.5 = 0.51176 atm
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