Maxwell Boltzmann Distribution Pogil Answer Key Extension Questions Repack 【99% SIMPLE】

Given that the fraction of molecules with kinetic energy greater than (E_a) is roughly ( e^-E_a / RT ), explain why a reaction with (E_a = 50 \text kJ/mol) proceeds very slowly at 300K but rapidly at 400K. (Use (R = 8.314 \text J/mol·K)).

The Maxwell-Boltzmann Distribution is a cornerstone of kinetic molecular theory, describing how speeds are spread out among particles in a gas. If you are working through a activity, you’ve likely mastered the basics of how temperature affects the "hump" of the graph. Given that the fraction of molecules with kinetic

would double. Since the y-axis represents the number of particles, having twice as many moles means there are twice as many particles at every possible speed. Khan Academy Extension Question 3: Activation Energy and Catalysts If you are working through a activity, you’ve

Slightly to the right of the peak. $$v_avg = \sqrt\frac8RT\pi M$$ Use this to find the mean of the molecular speeds. Khan Academy Extension Question 3: Activation Energy and

The shape and position of the curve remain the same because speed distribution depends on temperature and molar mass, not the total amount of gas. However, the area under the curve doubles because the total number of particles has doubled.