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Ideal Gas Equation

In a gaseous ...

Question

In a gaseous mixture at $20^{o}$ C, the total pressure $= 775$ torr. If the sum of the partial pressures of $H_{2}$ and $C O_{2}$ is $350$ torr and the partial volume of hydrogen $19.4 %$ , what is the partial pressure of $C O_{2}$ ?

225

torr

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300

torr

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275

torr

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200

torr

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Solution

The correct option is D $200$ torr
Partial volume= $X_{H_{2}} \times Total volume$
$∴ X_{H_{2}} = \frac{% partial volume}{100} = 0.194$
$P_{t} = 775 t o r r$ ,
$P_{H_{2}} + P_{C O_{2}} = 350 \Rightarrow X_{H_{2}} \times P_{t} + X_{C O_{2}} \times P_{t} = 350$
$∴ X_{H_{2}} + X_{C O_{2}} = \frac{350}{775} = 0.451$
$∴ X_{C O_{2}} = 0.451 - X_{H_{2}} = 0.257$
$P_{C O_{2}} = X_{C O_{2}} \times P_{t} = 0.257 \times 775 \approx 200 t o r r$

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In a gaseous mixture at 20oC, the total pressure =775 torr. If the sum of the partial pressures of H2 and CO2 is 350 torr and the partial volume of hydrogen 19.4%, what is the partial pressure of CO2?

The correct option is D 200 torrPartial volume= XH2×Total volume∴XH2=% partial volume100=0.194Pt=775torr,PH2+PCO2=350⇒XH2×Pt+XCO2×Pt=350∴XH2+XCO2=350775=0.451∴XCO2=0.451−XH2=0.257PCO2=XCO2×Pt=0.257×775≈200torr

In a gaseous mixture at $20^{o}$ C, the total pressure $= 775$ torr. If the sum of the partial pressures of $H_{2}$ and $C O_{2}$ is $350$ torr and the partial volume of hydrogen $19.4 %$ , what is the partial pressure of $C O_{2}$ ?