During an adiabatic process, if the pressure of a gas is found to be proportional to the cube of its absolute temperature, then the ratio of CVCP for the gas is :
To begin with, we're told that during an adiabatic process, the pressure P of a gas is directly proportional to the cube of its absolute temperature T, that is, P∝T3. From this, we can express the relation as P=kT3, where k is a constant.
In an adiabatic process, PVγ=constant, where γ=CVCP, P is the pressure, V is the volume, CP is the heat capacity at constant pressure, and CV is the heat capacity at constant volume.
Also, the ideal gas equation is PV=nRT, where n is the amount of substance, R is the ideal gas constant, and T is the absolute temperature. This can be rearranged to express P in terms of T and V, resulting in P=VnRT.
Given that P=kT3, we can equate this to the expression we got from the ideal gas law: VnRT=kT3. Simplifying, we get V=kT2nR, which shows that V is inversely proportional to T2.
Now, let's recall the adiabatic condition PVγ=constant. Substituting the proportionalities P∝T3 and V∝T−2 into this equation, it becomes T3(T−2)γ=constant, simplifying to T3−2γ=constant.
For the expression T3−2γ=constant to hold true in an adiabatic process, where the only variable is temperature T, the exponent must equal to zero (as the quantity of T to some power equals to a constant suggests that the change in T does not alter the value of the expression). This implies 3−2γ=0, solving for γ:
3−2γ=0⟹2γ=3⟹γ=23
Therefore, the ratio of CVCP for the gas is 23, which matches with Option B 23.














































