Oxygen and cyclopropane at partial pressures orf 570 torr and 170 torr respectively are mixed in a gas cylinder. What is the ratio of the number of moles of cyclopropane to the number of moles of oxygen?

\frac{170 \times 42}{570 \times 32} = 0.39

\frac{170}{24} / (\frac{170}{42} + \frac{570}{32}) \approx 0.19

\frac{170}{740} = 0.23

\frac{170}{570} = 0.30

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Oxygen and cyclopropane at partial pressures orf 570 torr and 170 torr respectively are mixed in a gas cylinder. What is the ratio of the number of moles of cyclopropane to the number of moles of oxygen?

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Text solutionVerified

According to ideal gas equation,

p_{1} V = n_{1} R T \dots .(i)

p_{2} V = n_{2} R T \dots (ii)

From Eqs. (i) and (ii)

\frac{p _{1} V}{p _{2} V} = \frac{n _{1} R T}{n _{2} R T} \Rightarrow \frac{p _{1}}{p _{2}} = \frac{n _{1}}{n _{2}}

\frac{n _{1}}{n _{2}} = \frac{p _{1}}{p _{2}} = \frac{170}{570} = 0.30

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Question Text	Oxygen and cyclopropane at partial pressures orf 570 torr and 170 torr respectively are mixed in a gas cylinder. What is the ratio of the number of moles of cyclopropane to the number of moles of oxygen?
Answer Type	Text solution:1
Upvotes	150

Oxygen and cyclopropane at partial pressures orf 570 torr and 170 torr respectively are mixed in a gas cylinder. What is the ratio of the number of moles of cyclopropane to the number of moles of oxygen?

Text solutionVerified

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