The work done in an adiabatic change in a gas depends only on

(1) Change is pressure

(2) Change is volume

(3) Change in temperature

(4) None of the above

In adiabatic expansion 

(1) ΔU = 0

(2) ΔU = negative

(3) ΔU = positive

(4) ΔW = zero

The pressure and density of a diatomic gas $(\gamma =7/5)$ changes adiabatically from (P, d) to (P', d'). If $\frac{d\text{'}}{d}=32$, then $\frac{P\text{'}}{P}$ should be: 

An ideal gas at 27°C is compressed adiabatically to $\frac{8}{27}$ of its original volume. If $\gamma =\frac{5}{3}$, then the rise in temperature is

(1) 450 K

(2) 375 K

(3) 225 K

(4) 405 K

Two identical samples of a gas are allowed to expand, (i) isothermally and (ii) adiabatically. The work done will be:

Which is the correct statement ?

(1) For an isothermal change PV = constant

(2) In an isothermal process the change in internal energy must be equal to the work done

(3) For an adiabatic change $\frac{P_2}{P_1}={\left(\frac{{\displaystyle V_2}}{{\displaystyle V_1}}\right)}^{\gamma }$, where γ is the ratio of specific heats

(4) In an adiabatic process work done must be equal to the heat entering the system

During the adiabatic expansion of 2 moles of a gas, the internal energy of the gas is found to decrease by 2 joules, the work done during the process by the gas will be equal to -

(1) 1 J

(2) –1 J

(3) 2 J

(4) – 2 J

If $\gamma$ denotes the ratio of two specific heats of a gas, the ratio of slopes of adiabatic and isothermal PV curves at their point of intersection is 

(1) $\frac{1}{\gamma }$

(2) $\gamma$

(3) $\gamma -1$

(4) $\gamma +1$

Air in a cylinder is suddenly compressed by a piston, which is then maintained at the same position. With the passage of time