Thermodynamics ...

Consider a cycle followed by an engine as shown in figure
1 to 2 is isothermal
2 to 3 is adiabatic
3 to 1 is adiabatic
Such a process does not exist because

Two moles of helium gas undergo a cyclic process as shown in figure. Assuming the gas to be ideal. The net work done by the gas is:

Some gas $$(\dfrac { { C }_{ p } }{ { C }_{ v } }$$ = $$\gamma$$ = 1.25) follows the cycle ABCDA as shown in the figure. The ratio of the energy given out by the gas to its surroundings during the isochoric section of the cycle to expansion work done during the isobaric section of the cycle is:

One mole of an ideal gas goes from an initial state A to final state B via two processes : It first undergoes isothermal expansion from volume  V  to  3V  and then its volume is reduced from 3V to V at constant pressure. The correct P-V diagram representing the two processes is:

The freezer in a refrigerator is located at the top section so that;

NA heat engine has an efficiency n.Temperatures of source and sink are each decreased by 100 K. The efficiency of the engine:

An engine has an efficiency of $$0.25$$ when the temperature of sink is reduced by $$58C$$, if its efficiency is doubled, then the temperature of the source is:

In a heat engine, the temperature of the source and sink is $$500 K$$ and $$375 K$$. If the engine consumes $$ 25\times{ 10 }^{ 5 }$$ per cycle, the work is done per cycle is:

A one mole of an ideal gas expands adiabatically at constant pressure such that its temperature T$$\propto \dfrac { 1 }{ \sqrt { V }}$$. The value of the adiabatic constant of gas is:

Two bars of same length and same cross -sectional area but of different thermal conductivities $$K_1$$ and $$K_2$$ are joined end to end as shown in the figure .One end of the compound bar is at temperature $$T_1$$ and the opposite end at temperature $$T_2$$ $$(where T_1 > T_2)$$.
The temperature of the junction is