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 (a) diatomic;

Video transcript

Welcome back everybody. We are given 1.4 moles of a di atomic gas and we are told that we want to increase its temperature by 38 Kelvin. And we are tasked with finding how much heat is going to be absorbed by the gas to achieve this increase in temperature. We have a formula for this. We have the heat absorbed is going to be easy to the number of moles times the molar heat capacity, times our desired change in temperature. Now we have these two terms already. But what is going to be the molar heat capacity for a di atomic gas or a di atomic gas? It is going to be equivalent to five halves times the ideal gas constant. I'm actually going to plug this into our formula right here we get that. The heat absorbed is now equal to the number of moles times five halves times the ideal gas constant, times our desired increase in temperature. So let's go ahead and plug in our numeric values here we have that this is equal to 1. moles, times five halves times 8. hour constant times 38 degrees kelvin. Which one? You multiply this In your calculator, you get that, this is 1,106 jewels corresponding to our final answer choice of B. Thank you all so much for watching. Hope this video helped. We will see you all in the next one