The pressure exerted by a non- reactive gaseous mixture of 6.4 g of methane and 8.8 g of carbon dioxide in a 10 L vessel at 27°C is _______ kPa. (Round off to the nearest integer).
[ Assume gases are ideal, R = 8.314 J mol-1 K-1 Atomic masses: C: 12.0 u, H: 1.0 u, O: 16.0 u]
The pressure exerted by a non- reactive gaseous mixture of 6.4 g of methane and 8.8 g of carbon dioxide in a 10 L vessel at 27°C is _______ kPa. (Round off to the nearest integer).
[ Assume gases are ideal, R = 8.314 J mol-1 K-1 Atomic masses: C: 12.0 u, H: 1.0 u, O: 16.0 u]
Mole of CH? = 6.4 / 16 = 0.4 and mole of CO? = 8.8 / 44 = 0.2
Total mole = (0.4 + 0.2) = 0.6 mole of a non-reacting mixture of gas
Using Ideal Gas Law; P = nRT / V
P = (0.6 * 8.314 * 300) / 10 = 149.65 kPa
Ans = 150 (Rounded off)
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