Calculate the change in internal energy of a gas which performs 150 joules of work on obtaining 15 cals of heat.

Open in App

Solution

Heat, $Q = 15 c a l$

Work done, $W = 150 J$

$1 c a l = 4.2 J$

From first law of thermodynamic

$Q = Δ U + W$

$Δ U = Q - W = 15 \times 4.2 - 150 = - 87 J$

Hence, decrease in potential energy is $87 J$

Suggest Corrections

Similar questions

Q. A gas absorbs 80 cal of heat. If the work done by the gas is 150 J, the change in internal energy is:

Q. A heat engine receives

150

Joules of heat energy and performs

70

Joules of work. If heat loss in the surrounding is zero. Find out by what value does the internal energy of the system change?

Find the change in the internal energy of a gas when it absorbs 80 calories of heat and performs work equal to 170 joules

A system performs $101.3 J$ of work on its surrounding and absorbs $15 K J$ of heat from surroundings. The change in internal energy of the system is:

In a thermodynamics process, pressure of a fixed mass of gas is changed in such a manner that the gas releases 30 joule of heat and 18 joule of work was done on the gas. If the initial internal energy of the gas was 60 joule, then the final internal energy will be

Join BYJU'S Learning Program

Calculate the change in internal energy of a gas which performs 150 joules of work on obtaining 15 cals of heat.

Heat, Q=15cal Work done, W=150J 1cal=4.2J From first law of thermodynamic Q=ΔU+W ΔU=Q−W=15×4.2−150=−87J Hence, decrease in potential energy is 87J

Heat, $Q = 15 c a l$

Work done, $W = 150 J$

$1 c a l = 4.2 J$

From first law of thermodynamic

$Q = Δ U + W$

$Δ U = Q - W = 15 \times 4.2 - 150 = - 87 J$

Hence, decrease in potential energy is $87 J$