An ideal gas undergoes an adiabatic expansion. Consider the following statements: A. Heat is absorbed by the gas. B. The temperature of the gas decreases. C. The gas does positive work. D. Internal energy of the gas increases. E. Heat exchanged with the surroundings is zero. Choose the correct answer from the options given below:

Step-by-step solution

For an adiabatic process, there is no heat exchange with the surroundings. Therefore, Q = 0 , which means statement E is correct and statement A is incorrect. Since the gas undergoes expansion, its volume increases. Thus, the work done by the gas is positive ( W > 0 ). This makes statement C correct. According to the first law of thermodynamics, Q = U + W . Substituting Q = 0 , we get U = -W . Since W is positive, U must be negative. A decrease in internal energy implies a decrease in the temperature of the ideal g