A 10 litre flask at 298 K contains a gaseous mixture of CO and CO2 at a total pressure of 2 atm- If 0-20 mole of CO is present find its partial pressure and also that of CO2-

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Standard XII

Chemistry

Charles' Law

A 10 litre ...

Question

A $10$ litre flask at $298 x K$ contains a gaseous mixture of $C O$ and $C O_{2}$ at a total pressure of $2 x a t m$ . If $0.20 x m o l e$ of $C O$ is present find its partial pressure and also that of $C O_{2}$ .

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Solution

Total moles = $\frac{P V}{R T}$
= $\frac{2 \times 10}{298 \times 0.0821}$
= $0.8174$
Moles of $C O_{2}$ = $0.8174 - 0.2 = 0.6174$
Partial pressure of $C O$ = $X_{C O} \times 2 = \frac{0.2}{0.8174} \times 2 = 0.4893 a t m$
Partial pressure of $C O_{2}$ = $2 - 0.4893 = 1.51 a t m$

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A 10 litre flask at 298xK contains a gaseous mixture of CO and CO2 at a total pressure of 2xatm. If 0.20xmole of CO is present find its partial pressure and also that of CO2.

Total moles = PVRT=2×10298×0.0821=0.8174Moles of CO2=0.8174−0.2=0.6174Partial pressure of CO= XCO×2=0.20.8174×2=0.4893 atmPartial pressure of CO2=2−0.4893=1.51 atm

A $10$ litre flask at $298 x K$ contains a gaseous mixture of $C O$ and $C O_{2}$ at a total pressure of $2 x a t m$ . If $0.20 x m o l e$ of $C O$ is present find its partial pressure and also that of $C O_{2}$ .

Total moles = $\frac{P V}{R T}$
= $\frac{2 \times 10}{298 \times 0.0821}$
= $0.8174$
Moles of $C O_{2}$ = $0.8174 - 0.2 = 0.6174$
Partial pressure of $C O$ = $X_{C O} \times 2 = \frac{0.2}{0.8174} \times 2 = 0.4893 a t m$
Partial pressure of $C O_{2}$ = $2 - 0.4893 = 1.51 a t m$