A0.877 mol sample of n2(g) initially at 298 k and 1.00 atm is held at constant volume while enough heat is applied to raise the temperature of the gas by 15.7 k. assuming ideal gas behavior, calculate the amount of heat in joules required to affect this temperature change and the total change in internal energy, δ note that some books use δ as the symbol for internal energy instead of δ

Answer : The value of is 286.2 J and 286.2 J respectively.

Explanation : Given,

Moles of sample = 0.877 mol

Change in temperature = 15.7 K

First we have to calculate the heat absorbed by the system.

Formula used :

where,

q = heat absorbed by the system = ?

n = moles of sample = 0.877 mol

= Change in temperature = 15.7 K

= heat capacity at constant volume of (diatomic molecule) =

R = gas constant = 8.314 J/mol.K

Now put all the given value in the above formula, we get:

Now we have to calculate the change in internal energy of the system.

As we know that, work done is zero at constant volume. So,

Therefore, the value of is 286.2 J and 286.2 J respectively.

the answer is to check all of them! they all apply well at least i think so!

answerscientific theory;