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Standard XII

Chemistry

Dalton's Law of Partial Pressures

Three caniste...

Question

Three canisters, A, B, and C, are all at the same temperature, with volumes of 2.0, 4.0, and 6.0 liters, respectively. Canister A contains 0.976 g of argon gas at a pressure of 120 torr, Canister B contains 1.37 g of nitrogen gas at a pressure of 210 torr, and canister C is completely empty at the start. Assuming ideality, what would the pressure become in canister C if the contents of A and B are completely transferred to C?

180 torr

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330 torr

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675 torr

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0.25 atm

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None of the above

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Solution

The correct option is B 180 torr
$n_{C} = n_{A} + n_{B}$
$P_{C} V_{C} = P_{A} V_{A} + P_{B} V_{B}$
$P C \times 6.0 L = 120 torr \times 2.0 L + 210 torr \times 4.0 L$
$P_{C} \times 6.0 L = 240 torr L + 840 torr L$
$P_{c} \times 6.0 L = 1080$ torr L
$P_{C} = 180$ torr

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Similar questions

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The correct option is B 180 torrnC=nA+nBPCVC=PAVA+PBVBPC×6.0L=120torr×2.0L+210torr×4.0LPC×6.0L=240torrL+840torrLPc×6.0L=1080 torr LPC=180torr

The correct option is B 180 torr
$n_{C} = n_{A} + n_{B}$
$P_{C} V_{C} = P_{A} V_{A} + P_{B} V_{B}$
$P C \times 6.0 L = 120 torr \times 2.0 L + 210 torr \times 4.0 L$
$P_{C} \times 6.0 L = 240 torr L + 840 torr L$
$P_{c} \times 6.0 L = 1080$ torr L
$P_{C} = 180$ torr