Be sure to answer all parts. A sample of natural gas contains 7.424 moles of methane (CH4), 0.691 moles of ethane (C2H6), and 0.243 moles of propane (C3H8). If the total pressure of the gases is 3.78 atm, what are the partial pressures of the gases

Explanation:

To solve this problem we need to keep in mind that the partial pressure of a gas is equal to the mole fraction of the gas multiplied by the total pressure of the mixture.

First we calculate the mole fraction of each gas:

Total number of moles = 7.424 + 0.691 + 0.243 = 8.358 moles

Now we calculate the partial pressure of each gas:

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation: