## Question

In an adiabatic expansion of a gas, the product of pressure and volume:

### Solution

Decreases

In an adiabatic expansion of a gas, temperature of the gas decreases.

Now,

#### SIMILAR QUESTIONS

If *R* is universal gas constant, the amount of heat needed to raise the temperature of 2 moles of an ideal mono-atomic gas from 273 K to 373 K when no work is done is:

The temperatures of inside and outside of a refrigerator are 273 K and 303 K respectively. Assuming that the refrigerator cycle is reversible, for every joule of work done, the heat delivered to the surroundings will be nearly:

In a thermodynamic process, pressure of a fixed mass of a gas is changed in such a manner that the gas releases 20 J of heat and 8 J of work is done on the gas. If initial internal energy of the gas was 30 J, what will be the final internal energy?

An ideal gas is taken through a cyclic thermo-dynamical process through four steps. The amounts of heat involved in these steps are:

respectively. The corresponding works involved are: respectively. The value of *W*_{4} is:

When an ideal diatomic gas is heated at constant pressure fraction of the heat energy supplied which increases the internal energy of the gas is:

70 calories of heat are required to raise the temperature of 2 moles of an ideal gas at constant pressure from 30^{o}C to 35^{o}C. The amount of heat required to raise the temperature of the same gas through same range (30^{o}C to 35^{o}C) at constant volume is:

A motor-car tyre has a pressure of 2 atmosphere at 27^{o}C. It suddenly bursts. If (*C _{p}/C_{v}*) = 1.4 for air, find the resulting temperature:

Find the amount of work done to increase the temperature of one mole of ideal gas by 30^{o}C, if it is expanding under the condition (*R* = 8.31 J/mol-K):

For an adiabatic expansion of a perfect gas, the value of is equal to:

One of the most efficient engines ever developed operates between 2100 K and 700 K. Its actual efficiency is 40%. What percentage of its maximum possible efficiency is this?