If 0.75 mole of cyclopropane and 0.66 mole of oxygen are mixed in vessel with a total pressure of 0.7 atmosphere, what is the partial pressure of oxygen in ...

The question involves finding the partial pressure of oxygen in a mixture of cyclopropane and oxygen. We are given the total pressure of the mixture, as well as the moles of each component. To solve this problem, we need to use the mole fraction of oxygen. The mole fraction is the number of moles of oxygen divided by the total number of moles in the mixture. First, we need to calculate the total number of moles in the mixture: Total moles = moles of cyclopropane + moles of oxygen Total moles = 0.75 + 0.66 Total moles = 1.41 Next, we can calculate the mole fraction of oxygen: Mole fraction of oxygen = moles of oxygen / total moles Mole fraction of oxygen = 0.66 / 1.41 Mole fraction of oxygen = 0.4681 Finally, we can calculate the partial pressure of oxygen using Dalton's law of partial pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gases in the mixture: Partial pressure of oxygen = mole fraction of oxygen x total pressure Partial pressure of oxygen = 0.4681 x 0.7 Partial pressure of oxygen = 0.3277 or approximately 0.33 atmosphere. Therefore, the correct answer is, 0.33 atmosphere.