A 8.40 L container holds a mixture of two gases at 35°C. The partial pressures o

Question

A 8.40 L container holds a mixture of two gases at 35°C. The partial pressures of gas A and gas B, respectively, are 0.194 ATM and 0.695 ATM. If 0.170 mol of a third gas is added with no change in volume or temperature, what will the total pressure become? A 8.40 L container holds a mixture of two gases at 35°C. The partial pressures of gas A and gas B, respectively, are 0.194 ATM and 0.695 ATM. If 0.170 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?

Explanation / Answer

Partial pressure of gas A ( Pa) = 0.194 atm

Partial pressure of gas B ( Pb) = 0.695 atm

Partial pressure of third gas added ( Pc ) = nRT/V = 0.170 x 0.0821 x 308 / 8.40 = 0.512 atm

Accoding to Graham's law of partial pressures,

toyal pressure = sum of the partial pressures of individual gases

=> PT = Pa + Pb + Pc = 0.194 + 0.695 + 0.512

=> PT = 1.401 atm   <<<<<<---------(ANSWER)

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