An ideal gas undergoes a process where its internal energy increases by $50\,J$ while $100\,J$ of heat is added to it. How much work is done by the gas during this process?

The state of a thermodynamic system is represented by

Which of the following can not determine the state of a thermodynamic system

The perfect gas goes from a state A to another state B by absorbing $8 imes {10^5}$J of heat and doing $6.5 imes {10^5}{\rm{J}}$of external work. It is now transferred between the same two states in another process in which it absorbs ${10^5}J$ of heat in the second process. Then

If earth suddenly stops rotating about its own axis, the increase in it’s temperature will be

Find the change in the entropy in the following process $100g$ of ice at ${0^ \circ }C$ melts when dropped in a bucket of water at ${50^ \circ }C$ (Assume temperature of water does not change)

A system absorbs 500 J of heat and does 200 J of work. What is the change in its internal energy?

The first law of thermodynamics is concerned with the conservation of

The state of a thermodynamic system is represented by

Six moles of ${{\rm{O}}_2}$ gas is heated from ${20^ \circ }C\;{\rm{to}}\;{35^ \circ }C$ at constant volume. If specific heat capacity at constant pressure is 8 cal ${\rm{mo}}{{\rm{l}}^{ - 1}} - {{\rm{K}}^{ - 1}}$ and $R = 8.31\;{\rm{Jmo}}{{\rm{l}}^{ - 1}} - {{\rm{K}}^{ - 1}}$, what is change in internal energy of gas?

A system does 100 J of work and its internal energy increases by 50 J. How much heat was added to the system?