A gas-phase mixture of H2 and N2 has a total pressure of 784 torr with an N2

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partial pressure of 124 torr. What mass of H2 gas is present in 2.00 L of the mixture at 298K?

Dec 15th, 2014

The partial pressure of H2=784-124=660 torr

PV=nRT

For H2, P=660 torr, V=2.00L, T=298K, R=62.36 L Torr K−1   mol−1

So n=PV/RT=660x2.00/(62.36x298)=0.071 mol

The mass of H2=2x0.071=0.142 g

Dec 15th, 2014

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