Consider a gas in a container, where all gas molecules have kinetic energy, a function of the molecule's mass and its velocity. The motion of the gas molecules is random in magnitude and direction; however, the average kinetic energy remains the same. Recall from the kinetic molecular theory that the average translational kinetic energy per molecule depends only on the temperature. Comparing the kinetic energy equations, rearranging the terms, and taking the square root on both sides relates the square root of the mean-square speed, also known as the root-mean-square or RMS speed. With every collision, the velocity of individual gas particles change. Therefore, a collection of gas molecules has a slightly asymmetric velocity distribution curve known as the Maxwell-Boltzmann distribution. The peak of the curve corresponds to the most probable velocity, which is less than the RMS speed. A plot of the velocity distribution for any gas at different temperatures displays an increase in the RMS speed and a broadening of the speed distribution at higher temperatures.