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ivolga24 [154]
3 years ago
5

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.)

Chemistry
1 answer:
aivan3 [116]3 years ago
6 0

Answer: the molar Mass of the unknown gas is 367.12

Explanation:Please see attachment for explanation

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Explanation:

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<u>Data:</u>

M1 = 6.01 M stock solution concentration

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24H2S + 16HNO3 3Sg+ 16NO + 32H2O
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