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:
As given,
$$\dfrac{P}{V}=PV^{-1}=constant$$
Hence, polytropic exponent is $$-1$$
In a polytropic process,
$$\Delta Q = \Delta U + W=( \dfrac{R}{\gamma -1}- \dfrac{R}{\eta -1})\Delta T$$ where $$\eta= -1$$ is the polytropic exponent.
$$ \therefore \Delta Q = R(\dfrac{1}{\dfrac{5}{3}-1}- \dfrac{1}{-1-1})(2T_0 - T_0)=2RT_0$$
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).
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 :
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 :
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?