G2.3 mol of monatomic gas a initially has 4800 j of thermal energy. it interacts with 2.9 mol of monatomic gas b, which initially has 8500 j of thermal energy. part a which gas has the higher initial temperature?

To determine the gas which has the higher initial temperature, we need an equation that would relate energy and temperature. From thermodynamics, we use the expression Energy = nCvT where n is the number of moles, Cv is the heat capacity at constant volume and T is the temperature. By evaluating the temperature of both gases we determine the which would have higher temperature.

4800 = 2.3CvT
T = 2086.96/Cv

8500 = 2.9CvT
T = 2931.03/Cv

Assuming that both gases are the same. Therefore, the value of Cv for both would be equal. So, we conclude that it is the second gas with 2.9 moles would have the higher initial temperature.

Uncle grandma

There is no graph to look at on here, but i shall explain them to you. a line graph is just in its title it’s a graph with a line running through the dots to show an increase or decrease. a bar graph is used to show how much or how little something is so a comparison. a scatter plot is used to graph points to tell the data. and i don’t know what a histogram is.