JAMB - Chemistry (1985 - No. 8)
In the reaction H2(g)O \(\to\) H2(g) + 1/2O2(g)
ΔH = -2436000 KJ, which of the following has no effect on the equilibrium position?
ΔH = -2436000 KJ, which of the following has no effect on the equilibrium position?
Adding argon to the system
Lowering the temperature
Adding hydrogen to the system
Decreasing the pressure
Increasing the temperature
Wyjaśnienie
The equilibrium position of a reversible reaction can be shifted by changes in concentration, pressure, and temperature, as dictated by Le Chatelier's principle, which states that the system will adjust to counteract the applied change.
For the fact that Argon is not one of the reactants or products, even if its function is to act as a catalyst, it still wouldn't have any effect on the chemical system in equilibrium.