Daily Problem #15 1. A mixture of gases contains 0.31 mol CH, 0.25 mol C2Ho, and
ID: 547664 • 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
Ans 1 :
The partial pressure of the gas is directly proportional to its mole fraction (x) in the mixture.
xCH4 = 0.31 / (0.31 + 0.25 + 0.29) = 0.3647
xC2H6 = 0.31 / (0.31 + 0.25 + 0.29) = 0.2941
xC3H8 = 0.29 / (0.31 + 0.25 + 0.29) = 0.3412
So the partial pressure of gases will be :
pCH4 = 0.3647 x 1.50 = 0.547 atm
pC2H6 = 0.2941 x 1.50 = 0.441 atm
pC3H8 =0.3412 x 1.50 = 0.512 atm
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