Final answer:
Pressure can change without altering temperature if a reaction involves gas and there's a change in the number of moles of gas, as this will affect the equilibrium position according to Le Chatelier's principle. So, the correct option is A.
Step-by-step explanation:
The pressure of a chemical reaction can indeed change without affecting the temperature under specific conditions. Answer A) Yes, pressure can change without affecting the temperature, is the correct choice for this question. According to Le Chatelier's principle, if the reaction involves gases and there is a change in the total number of moles of gas, a change in pressure or volume will affect the equilibrium of the system even at constant temperature. This is because changes in pressure can change the partial pressures of the gases involved in the reaction, shifting the reaction's equilibrium position. For instance, if a reaction has more moles of gas on the product side than on the reactant side, an increase in pressure will shift the equilibrium towards the reactants to reduce the number of gas moles, thereby reducing the pressure. Conversely, a decrease in pressure would shift the equilibrium towards more gas production, i.e., towards the products. This demonstrates that changes in pressure, independent of temperature, can indeed affect a chemical equilibrium.