Final answer:
Without sufficient context or a diagram to clarify points E, F, and A, a specific answer regarding pressure changes at these points cannot be provided. In general thermodynamics, when energy is added to a gas in a constant volume, pressure increases; for gases in equilibrium, changes in temperature, pressure, and concentration can shift the equilibrium.
Step-by-step explanation:
The original question appears to contain elements related to the behavior of gases under different conditions, which suggests it pertains to the principles of Physics, particularly within the topic of thermodynamics. Unfortunately, without more context or a diagram that specifies what points E, F, and A refer to, it's challenging to provide a definitive answer. However, considering general principles, when heat adds energy to a system, it typically increases the pressure if the volume is constant or able to expand freely (Gay-Lussac's Law). If the system is forced to stay in a constant volume, the pressure would increase even if more gas is added.
For gases in equilibrium, adding heat (increased temperature) or adding more gas, such as H2, usually shifts the equilibrium towards the products if we are considering a typical exothermic reaction. On the opposite, decreased pressure generally shifts the equilibrium towards the side with more moles of gas. If these principles are applied to points E and F without additional specifics, it is not possible to determine whether pressures at points E and F increase, decrease, or remain the same as it depends on the system's conditions and constraints.
Finally, gas moves from an area of high pressure to an area of low pressure, and when the masses of particles within a closed system remain the same and energy is added, typically the temperature of the system increases.