Determine the pressure exerted by a mixture of 6.4 text g of methane (CH_ 4 ) and 8.8 text g of carbon dioxide (CO_ 2 ) confined in a 10 text L vessel at 27^ circ text C . [Use R = 8.314 text J mol ^ -1 text K ^ -1 ]

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EEJ MAIN Chemistry QUESTION #7178

Question 1

Determine the pressure exerted by a mixture of $6.4 \text{ g}$ of methane ($CH_{4}$) and $8.8 \text{ g}$ of carbon dioxide ($CO_{2}$) confined in a $10 \text{ L}$ vessel at $27^{\circ}\text{C}$. [Use $R = 8.314 \text{ J mol}^{-1}\text{K}^{-1}$]

$125 \text{ kPa}$
$150 \text{ kPa}$✔️
$210 \text{ kPa}$
$100 \text{ kPa}$

Correct Answer Explanation

First, calculate the total moles ($n$):

Moles of $CH_{4} = 6.4 / 16 = 0.4 \text{ mol}$
Moles of $CO_{2} = 8.8 / 44 = 0.2 \text{ mol}$
Total $n = 0.6 \text{ mol}$
Using $P = \frac{nRT}{V}$:
$P = \frac{0.6 \times 8.314 \times 300}{10 \times 10^{-3} \text{ m}^{3}}$
$P \approx 149,652 \text{ Pa} \approx 150 \text{ kPa}$

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