Question

A 2 litre flask contain 1.6gm Methan and 0.5gm hydrogen at 27c calculate the partial pressure of each gas in the mixture and hence calculate the total pressure

Answer 1

Answer the Question #79429

V=2 l.

$m_{(CH4)} = 1.6\ \text{g}$

$m_{(H2)} = 0.5\ \text{g}$

$T = 27^{\circ} \text{C} = 300\ \text{K}$

$P_{(CH4)} = ?$

$P_{(H2)} = ?$

$P_{\text{tot}} = ?$

Formula: $PV = (mRT)/M$ therefore $P = (mRT)/MV$

and $P_{\text{tot}} = P_{(CH4)} + P_{(H2)}$

$P_{(CH4)} = (1.6 \times 8.314 \times 300) / (16 \times 2) = 124.71\ \text{kpa}$

$P_{(H2)} = (0.5 \times 8.314 \times 300) / (2 \times 2) = 311.775\ \text{kpa}$

$P_{\text{tot}} = 124.71 + 311.775 = 436.485$