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the partial pressure of carbon dioxide in a mixture in 0.31 if the mole fraction of the carbon dioxide is 0.46 what is the total pressure of the mixture
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To find the total pressure of the mixture, we first need to use the partial pressure and mole fraction of carbon dioxide to calculate the total moles of gas in the mixture.
Given:
Partial pressure of carbon dioxide (P_CO2) = 0.31 atm
Mole fraction of carbon dioxide (X_CO2) = 0.46
From the ideal gas law, we know that the partial pressure of a gas is equal to the mole fraction of the gas multiplied by the total pressure:
P_CO2 = X_CO2 * P_total
Rearranging the equation to solve for the total pressure:
P_total = P_CO2 / X_CO2
P_total = 0.31 / 0.46
P_total = 0.67391304348 atm
Therefore, the total pressure of the mixture is approximately 0.67 atm.