What is the average kinetic energy per particle in 1.00 mole of an ideal gas at a pressure of 1.50 atmospheres and a volume of 2.00 liters? A) 5.35 × 10^-22 J B) 6.02 × 10^-22 J C) 6.67 × 10^-22 J D) 7.57 × 10^-22 J E) 8.24 × 10^-22 J

Question

Quizplus · Accepted Answer

The average kinetic energy per particle in an ideal gas is given by the equation:$$KE = (3/2)kT$$where k is the Boltzmann constant and T is the temperature. The temperature can be calculated using the ideal gas law:$$PV = nRT$$where P is the pressure, V is the volume, n is the number of moles, and R is the ideal gas constant. Substituting the given values into these equations, we get:$$T = PV/nR = (1.50 ext{ atm})(2.00 ext{ L})/(1.00 ext{ mol})(0.0821 ext{ L atm/mol K}) = 36.6 ext{ K}$$$$KE = (3/2)kT = (3/2)(1.38 imes 10^{-23} ext{ J/K})(36.6 ext{ K}) = 7.57 imes 10^{-22} ext{ J}$$Therefore, the average kinetic energy per particle in 1.00 mole of an ideal gas at a pressure of 1.50 atmospheres and a volume of 2.00 liters is 7.57 × 10^-22 J.

What Is the Average Kinetic Energy Per Particle in 1