A gas of unknown molecular mass was allowed to effuse through a small opening under constant-pressure conditions. It required 10
5 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 31 s for 1.0 L of O2 gas to effuse. Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; in other words, rate is the amount that diffuses over the time it takes to diffuse.)
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Answer: 42.14 g
Explanation: calcium nitrate -
, the molar mass of calcium nitrate = 164 g
<h3> formula used = mass required =
= g