Final answer:
To find the partial pressures of gases A and B in the mixture, we need to determine their mole fractions. The mole fraction of A is 0.75 and the mole fraction of B is 0.25. Using Dalton's law of partial pressures, we can calculate the partial pressures of A and B to be 1.31 atm and 0.44 atm respectively.
Step-by-step explanation:
According to Dalton's law of partial pressures, the total pressure of a gas mixture is equal to the sum of the partial pressures exerted by each component. In this case, 2.50 mol of gas A is mixed with 0.85 mol of gas B, resulting in a final pressure of 1.75 atm. To find the partial pressures of A and B, we need to determine their mole fractions.
The mole fraction of A is calculated by dividing the moles of A by the total moles of both gases: XA = (2.50 mol)/(2.50 mol + 0.85 mol) = 0.75.
The mole fraction of B is calculated similarly: XB = (0.85 mol)/(2.50 mol + 0.85 mol) = 0.25.
The partial pressure of A is then determined by multiplying the mole fraction of A by the total pressure: PA = 0.75 * 1.75 atm = 1.31 atm.
The partial pressure of B is calculated similarly: PB = 0.25 * 1.75 atm = 0.44 atm.