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(B) According to Dalton's Law of Partial Pressures, the partial pressure of a gas is given by the product of its mole fraction and the total pressure

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$6$

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(B) According to Dalton's Law of Partial Pressures, the partial pressure of a gas is given by the product of its mole fraction and the total pressure of the mixture.$P_C = \chi_C 	imes P_{	ext{total}}$Where $\chi_C$ is the mole fraction of gas $C$.Total moles of gas $= 2 + 3 + 5 + 10 = 20 \ 	ext{moles}$.Moles of $C = 5 \ 	ext{moles}$.Mole fraction of $C$ $(\chi_C)$ $= \frac{5}{20} = 0.25$.Given $P_C = 1.5 \ atm$.$1.5 = 0.25 	imes P_{	ext{total}}$.$P_{	ext{total}} = \frac{1.5}{0.25} = 6 \ atm$.

$A$ gaseous mixture of $2$ moles of $A$, $3$ moles of $B$, $5$ moles of $C$, and $10$ moles of $D$ is contained in a vessel. Assuming that gases are ideal and the partial pressure of $C$ is $1.5 \ atm$, what is the total pressure (in $atm$)?

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