Question

A 6.60 L cylinder contains 2.94 mol of gas A and 3.28 mol of gas B, at a temp of 33.5 C. Calculate the partial pressure of each gas in the cylinder. Assume ideal gas behavior.

Answer 1

To calculate the partial pressure of each gas in the cylinder, divide the number of moles of each gas by the total volume and multiply by the gas constant and the temperature.

Step-by-step explanation:

To calculate the partial pressure of each gas in the cylinder, we can use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

First, let's calculate the total number of moles of gas in the cylinder by adding the moles of gas A and gas B: 2.94 mol + 3.28 mol = 6.22 mol.

Next, we can calculate the partial pressures of gas A and gas B by dividing the number of moles of each gas by the total volume of the cylinder and multiplying by the gas constant and the temperature: PA = (2.94 mol / 6.60 L) * (0.0821 atm L / mol K) * (33.5 + 273.15 K) = 2.07 atm; PB = (3.28 mol / 6.60 L) * (0.0821 atm L / mol K) * (33.5 + 273.15 K) = 2.31 atm.