One mole of an ideal monatomic gas undergoes a process described by the equation $$PV^3=$$constant. The heat capacity of the gas during this process is :
$$PV^*=$$ constant (Polytropic process)
Heat capacity in polytropic process is given by
$$[C=C_V+\dfrac{R}{1-x}]$$
Given that $$PV^3=constant\Rightarrow x=3$$ ......(1)
Also gas is monoatomic so $$C_V=\dfrac{3}{2}R$$ .......(2)
By formula
$$C=\dfrac{3}{2}R+\dfrac{R}{1-3}=\dfrac{3}{2}R-\dfrac{R}{2}=R$$
Hence, option A is correct
An ideal gas undergoes a quasi static, reversible process in which its molar heat capacity $$C$$ remains constant. If during this process the relation of pressure $$P$$ and volume $$V$$ is given by $$PV^n=$$constant, then $$n$$ is given by (Here $$C_P$$ and $$C_V$$ are molar specific heat at constant pressure and constant volume, respectively).
An ideal gas $$(C_p/C_v = \gamma)$$ is taken through a process in which the pressure and the volume vary as $$P= aV^b$$. Find the value of $$b$$ for which the specific heat capacity in the process is zero.
In a polytropic process $$PV^n =$$ constant :
In a given process for ideal gas, $$dW=0$$ and $$dH > 0$$. Then for the gas :
One mole of an ideal monoatomic gas at temperature $$T_o$$ expands slowly according to the law $$\dfrac{P}{V}= constant$$. If the final temperature is $$2T_o$$, heat supplied to the gas is:
A certain ideal gas undergoes a polytropic process $$PV^n = constant$$ such that the molar specific heat during the process is negative. If the ratio of the specific heats of the gas be $$\gamma$$, then the range of values of n will be
A sample of gas follows process represented by $$PV^2 = constant$$. Bulk modulus for this process is B, then which of the following graph is/are correct?