Thermodynamics ...

If R = universal gas constant, the amount of heat needed to raise the temperature of 2 moles of an ideal monoatomic gas from 273K to 373K when no work is done

An ideal gas is made to go through a cyclic thermodynamical process in four steps. The amount of heat involved are Q₁ = 600 J, Q₂ = – 400 J , Q₃ = – 300 J and Q₄ = 200 J respectively. The corresponding work involved are W₁ = 300 J, W₂ = – 200 J, W₃ = –150 J and W₄. What is the value of W₄?

A container of volume 1m³ is divided into two equal compartments by a partition. One of these compartments contains an ideal gas at 300 K. The other compartment is vacuum. The whole system is thermally isolated from its surroundings. The partition is removed and the gas expands to occupy the whole volume of the container. Its temperature now would be

110 J of heat is added to a gaseous system, whose internal energy change is 40 J, then the amount of external work done is

A thermo-dynamical system is changed from state (P₁, V₁) to (P₂, V₂) by two different process. The quantity which will remain same will be.

When two bodies A and B are in thermal equilibrium

For free expansion of the gas which of the following is true?

Which of the following cannot determine the state of a thermodynamic system?

The specific heat of hydrogen gas at constant pressure is C_P = 3.4 × 10³ cal/kg °C and at constant volume is C_V = 2.4 × 10³ cal/kg °C . If one kilogram hydrogen gas is heated from 10°C to 20°C at constant pressure, the external work done on the gas to maintain it at constant pressure is

In a thermodynamic process, pressure of a fixed mass of a gas is changed in such a manner that the gas molecules gives out 20 J of heat and 10 J of work is done on the gas. If the initial internal energy of the gas was 40 J, then the final internal energy will be