How much heat does it take to increase the temperature of 1.80 mol of an ideal gas by 50.0 K near room temperature if the gas is held at constant volume and is (b) monatomic?

Video transcript

Welcome back everybody. We are taking a look and are given 2. moles of a mono atomic gas inside of a container of constant volume. Now we want to increase the temperature by Kelvin and we are tasked with finding how much heat we need to supply to it to make that happen. Well, there's a formula for this. We have, the amount of heat we need to supply is equivalent to the number of moles times the molar heat capacity, times our desired change in temperature. Now we have these end terms right here. What is the molar heat capacity? Well, for a mono atomic gas, you're going to have that. It's equal to three halves times are ideal gas constant. I'm actually going to sub this in for our tv term right here and we get that Q. Is equal to end. Times three half times are times our delta T. So let's go ahead and plug in our values here we have 2.5 moles times three half Time is the ideal gas constant of 8.314 times our desired temperature change of 44 Kelvin. And when you multiply the cost, we get that. The amount of heat we need to supply is duels corresponding to answer choice. D thank you all so much for watching. Hope this video helped. We will see you all in the next one