A mixture of 10.0 g of Ne and 10.0 g Ar have a total pressure of 1.6 atm.What is the partial pressure of Ne?
A) 1.1 atm
B) 0.80 atm
C) 0.54 atm
D) 0.40 atm
E) 1.3 atm

Question

Quizplus · Accepted Answer

Dalton's law of partial pressures states that the total pressure of a mixture of non-reacting gases 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, the partial pressure of Ne can be calculated using the following formula:P(Ne) = (n(Ne) / n(total)) * P(total)where:P(Ne) is the partial pressure of Nen(Ne) is the number of moles of Nen(total) is the total number of moles of gasP(total) is the total pressureWe can first calculate the total number of moles of gas in the mixture:n(total) = n(Ne) + n(Ar)where:n(Ne) is the number of moles of Nen(Ar) is the number of moles of ArWe can then calculate the number of moles of each gas using the following formula:n = m / Mwhere:n is the number of molesm is the massM is the molar massThe molar mass of Ne is 20.18 g/mol and the molar mass of Ar is 39.95 g/mol. Therefore, the number of moles of Ne and Ar are:n(Ne) = 10.0 g / 20.18 g/mol = 0.496 moln(Ar) = 10.0 g / 39.95 g/mol = 0.250 molTherefore, the total number of moles of gas in the mixture is:n(total) = 0.496 mol + 0.250 mol = 0.746 molFinally, we can calculate the partial pressure of Ne:P(Ne) = (0.496 mol / 0.746 mol) * 1.6 atm = 1.1 atmTherefore, the partial pressure of Ne is 1.1 atm.

A Mixture of 10