For the same fractional increase in volume the final pressure is lower, so the temperature must have decreased rather than staying constant. It's equivalent to what you did mathematically, but I like the way you did it better.Vibhor said:
There is no need to invoke internal energy or the first law to address this problem. This can be done strictly as an ideal gas equation analysis.andrevdh said:
I saw it, but I wasn't able to figure out exactly what they are asking.Vibhor said:
TSny said:
.The answer to this question depends on the specific gas in question and the conditions it is undergoing. Generally, if the gas is in a closed system and no external energy is being added or removed, the gas will cool as it expands and heats as it is compressed. However, if energy is being added (e.g. through a heat source) or removed (e.g. through a refrigeration system), the gas can be heated or cooled intentionally.
When a gas is heated, the average kinetic energy of its molecules increases, causing them to move faster and collide with each other more frequently. This results in an increase in temperature. On the other hand, when a gas is cooled, the average kinetic energy of its molecules decreases, causing them to move slower and collide with each other less frequently. This results in a decrease in temperature.
According to the ideal gas law, the pressure of a gas is directly proportional to its temperature, assuming the volume and number of gas molecules stay constant. This means that as the temperature of a gas increases, its pressure will also increase, and vice versa.
When a gas is heated, its volume will increase as the molecules move faster and take up more space. On the other hand, when a gas is cooled, its volume will decrease as the molecules move slower and take up less space. This is because the volume of a gas is directly proportional to its temperature, assuming the pressure and number of gas molecules stay constant.
In a closed system, a gas cannot be both heated and cooled simultaneously. This is because the addition of heat will raise the temperature and increase the average kinetic energy of the molecules, while the removal of heat will lower the temperature and decrease the average kinetic energy. However, in certain situations, different parts of a gas may experience heating and cooling simultaneously, such as in a non-uniform gas flow with varying temperatures.
