In a mixture of CO_2 and CH_4 in a closed ves | vedclass

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(A) According to Dalton's Law of Partial Pressures,the total pressure $(P_{total})$ of a mixture of non-reacting gases is equal to the sum of their pa

Vedclass · Accepted Answer

$5.5 	imes 10^4 \, Pa$

Vedclass · Answer

(A) According to Dalton's Law of Partial Pressures,the total pressure $(P_{total})$ of a mixture of non-reacting gases is equal to the sum of their partial pressures. $P_{total} = P_{CO_2} + P_{CH_4}$ Given: $P_{total} = 8.3 	imes 10^4 \, Pa$ $P_{CO_2} = 2.8 	imes 10^4 \, Pa$ Substituting the values: $8.3 	imes 10^4 \, Pa = 2.8 	imes 10^4 \, Pa + P_{CH_4}$ $P_{CH_4} = (8.3 - 2.8) 	imes 10^4 \, Pa$ $P_{CH_4} = 5.5 	imes 10^4 \, Pa$

In a mixture of $CO_2$ and $CH_4$ in a closed vessel at a constant temperature,the total pressure is $8.3 \times 10^4 \, Pa$. If the partial pressure of $CO_2$ is $2.8 \times 10^4 \, Pa$,what will be the partial pressure of $CH_4$?

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