A gas mixture contains CO,Ar and H₂.What is the total pressure of the mixture,if the mole fraction of H₂ is 0.350 and the pressure of H₂ is 0.480 atm?

Question

Quizplus · Accepted Answer

Dalton's law of partial pressures states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas. The partial pressure of a gas is the pressure that the gas would exert if it occupied the entire volume alone.In this case, we are given the mole fraction of H2 and the pressure of H2. We can use the mole fraction to calculate the partial pressure of H2 using the following equation:Partial pressure of H2 = Mole fraction of H2 * Total pressureSubstituting the given values into the equation, we get:Partial pressure of H2 = 0.350 * Total pressureWe are also given that the partial pressure of H2 is 0.480 atm. Therefore, we can solve for the total pressure by rearranging the equation as follows:Total pressure = Partial pressure of H2 / Mole fraction of H2Substituting the given values into the equation, we get:Total pressure = 0.480 atm / 0.350 = 1.37 atmTherefore, the total pressure of the gas mixture is 1.37 atm.

A Gas Mixture Contains CO,Ar and H2

A Gas Mixture Contains CO,Ar and H₂