Question

A mixture of 8.1 g CH₄ and 8.1 g Kr is placed in a container, and the total pressure is found to be 0.38 atm.

Find the partial pressure of CH₄.
a) 0.19 atm
b) 0.21 atm
c) 0.38 atm
d) 0.76 atm

Answer 1

To find the partial pressure of CH₄ in a mixture of CH₄ and Kr gases, we first calculate the mole fraction of CH₄ and use it to calculate the partial pressure.

Step-by-step explanation:

According to Dalton's law of partial pressures, the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas. In this case, we have a mixture of CH₄ and Kr gases. Since the total pressure is given as 0.38 atm, we need to find the partial pressure of CH₄.

To find the partial pressure of CH₄, we first need to determine the mole fraction of CH₄ in the mixture. The mole fraction is the ratio of moles of a gas to the total moles of all gases in the mixture. We can calculate the moles of CH₄ and Kr using their respective masses and molar masses.

Once we have the moles of CH₄ and Kr, we can calculate their mole fractions. The mole fraction of CH₄ is then used to calculate the partial pressure of CH₄ by multiplying it by the total pressure of the mixture.