Consider the following reaction at equilibrium:

2NH3 (g)<-> N2 (g) + 3H2 (g) ΔH° = +92.4 kJ
Le Cha
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telier's principle predicts that increasing the temperature will shift the reaction to the.
a) stays same b)leftc)none d)right

As the ΔH° = +92.4 kJ

Q>0
Then the direct reaction is endothermic which means that increasing the temperature will shift the reaction to the right

Well, Le Châtelier's principle is like the Goldilocks of reactions. It always wants to find the perfect balance. So, let's see here. If we increase the temperature, that's like turning up the heat in a room. Things start to get a little uncomfortable, don't they? In this case, with +92.4 kJ of heat being released, I imagine the reaction would start sweating, thinking "Phew, it's getting hot in here!"

To restore that perfect balance, the reaction would want to cool down. So, based on Le Châtelier's principle, it would shift to the left, away from the heat, like a person moving away from a blazing fire. So, I hope you're ready to say "b) left" because that's the answer!

According to Le Chatelier's principle, if the temperature of a system at equilibrium is increased, the equilibrium will shift in the direction that consumes heat in order to counteract the temperature increase.

In this case, the reaction is exothermic as indicated by the positive value for ΔH°. This means that heat is released when the reaction occurs.

To counteract the temperature increase, the equilibrium will shift in the direction that consumes heat, which is the left side of the reaction.

Therefore, the answer is (b) left.

To determine the effect of increasing the temperature on the direction of the reaction, we need to consider Le Chatelier's Principle. According to this principle, if a stress is applied to a system at equilibrium, the system will adjust in such a way as to counteract the applied stress and restore equilibrium.

In this case, increasing the temperature is considered a stress on the system. To determine how the system will respond, we need to remember that the reaction is exothermic because the enthalpy change (ΔH°) is positive (+92.4 kJ). This means that the reaction releases heat as it proceeds from left to right (NH3 to N2 and H2).

By increasing the temperature, we are adding additional heat to the system. In response to this added heat, Le Chatelier's Principle states that the system will shift in the direction that absorbs heat. In other words, the equilibrium will shift to the left, favoring the reactants side to absorb the excess heat.

Therefore, the correct answer is (b) left. Increasing the temperature will shift the equilibrium to the left, favoring the formation of NH3 gas, while reducing the concentrations of N2 and H2 gases.