5.18. 2.9 g of a gas at 95°C occupied the same volume as 0.184 g of hydrogen at 17°C at the same pressure. What is the molar mass of the gas?

<p><strong>5.18.&nbsp;</strong>Given, P₁ = P₂ and V₁ = V₂</p><p>We know that P₁V₁ = P₂V₂</p><p>Or, &nbsp;&nbsp;&nbsp;&nbsp;&nbsp; &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;n₁RT₁ = n₂RT₂</p><p>i.e., &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; n₁T₁ = n₂T₂</p><p>_&nbsp;Substituting n = w/M, we get</p><p> (W₁/M₁) x T₁ = (W₂/M₂) x T₂</p><p> (2.9/M₁) x (95 + 273) = (0.184/2) x (17 + 273)</p><p>M₁ = (2.9 x 368 x 2) / (0.184 x 290) = 40 g mol^-1</p>

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