An ideal gas is subjected to a thermodynamic process `PV^(2//5)=0.40` where P is in Pa and V is in `m^(3)`. What is the slope of the P-V curve with volume plotted against x-axis at V=1 `m^(3)`?

Two moles of oxygen gas undergo a process given by P=2/(1+(V/3)^2 , where P is pressure and V is volume. What will be rms speed of gas molecules when volume of gas becomes 3 m^3 ?

What is the shape of the curve obtained on plotting P against PV at constant temperature for an ideal gas ?

An ideal gas undergoes a cyclic process (V,P) to (3 V, P) to (V, 4P) to (V, P) along straight lines on the P - V plane. Calculate the work done in the process.

An ideal monoatomic gas follows a thermodynamic process as shown in pressure-volume (P-V) plot. The work done in process AB is

If n moles of an ideal gas undergoes a thermodynamic process P=P_0[1+((2V_0)/V)^2]^(-1) , then change in temperature of the gas when volume is changed from V=V_0 to V=2V_0 is [Assume P_0 and V_0 are constants]

An ideal gas follows a process PV^(gamma) = constant where gamma = adiabatic exponent.The slope of P-V graph will be represented by

One mole of an ideal gas undergoes a process P = P_(0) [1 + ((2 V_(0))/(V))^(2)]^(-1) , where P_(0) V_(0) are constants. Change in temperature of the gas when volume is changed from V = V_(0) to V = 2 V_(0) is: