1. For an ideal gas, the average translational kinetic energy per molecule is $\bar K = \frac{3}{2}kT$ So it depends only on temperature, not directly on pressure or volume.

2. Now check each statement:

   (A) The average kinetic energy of a gas molecule decreases when the temperature is reduced.
   Since $\bar K \propto T$, lowering $T$ lowers average kinetic energy.
   (A) is true.

   (B) The average kinetic energy of a gas molecule increases with increase in pressure at constant temperature.
   At constant temperature, $\bar K = \frac{3}{2}kT$ remains unchanged. So changing pressure at constant $T$ does not change average kinetic energy.
   (B) is false.

   (C) The average kinetic energy of a gas molecule decreases with increase in volume.
   Average kinetic energy does not depend directly on volume; it depends only on temperature.
   (C) is false.

   (D) Pressure of a gas increases with increase in temperature at constant pressure.
   This statement is self-contradictory: if pressure is constant, it cannot increase.
   (D) is false.

   (E) The volume of gas decreases with increase in temperature.
   By Charles' law, at constant pressure, $V \propto T$ so volume increases with temperature, not decreases.
   (E) is false.

3. Therefore, only statement (A) is correct.

4. Compare with options:

• A: (A) and (D) only → false
• B: (A), (B) and (D) only → false
• C: (B) and (D) only → false
• D: (A), (B) and (E) only → false

So the correct conclusion is: none of the given options matches.

5. Since the stored correct answer is blank, I cannot agree with any provided stored option. The physically correct answer is only (A).