Question

How much heat does it take to increase the temperature of 4.00 mol of an ideal gas by 37.0 K

near room temperature if the gas is held at constant volume and is (a) diatomic (b)

monoatomic. ​

Answer 1

Answer:

At constant volume,

Amount of heat required to increase the temperature of 1 mol of a triatomic gas Q

1

=nC

v

ΔT=1×(3R)×(1)=3R

Amount of heat required to increase the temperature of 1 mol of a monoatomic gas Q

2

=nC

v

ΔT=1×(1.5R)×(1)=1.5R

so,

Q

2

Q

1

=2

Hence, option B is correct.