Consider the following reaction at equilibrium:

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

i was told right by some people and left by some people.???

See my response to your other post; or perhaps you are taking a vote on which way to answer. :-)

To determine the effect of increasing temperature on the equilibrium position of a reaction, we need to consider the reaction's enthalpy change (∆H°) and Le Chatelier's principle.

In this case, the reaction is endothermic, as indicated by the positive ∆H° value (+92.4 kJ). According to Le Chatelier's principle, increasing the temperature will favor the endothermic reaction, which means it will shift in the direction that consumes heat.

To understand this concept, remember that the reaction can be seen as having two opposite processes: the forward reaction (2NH3 ➝ N2 + 3H2) and the reverse reaction (N2 + 3H2 ➝ 2NH3). Increasing the temperature will provide more energy for the reactant particles, increasing the likelihood of successful collisions. Consequently, the reaction will shift in the direction that consumes heat, i.e., the endothermic forward reaction.

Therefore, increasing the temperature will cause the equilibrium position of the reaction to shift to the right (d) because the forward reaction is favored.

It's worth noting that the equilibrium position can also be influenced by other factors, such as changes in concentration, pressure, or the addition of a catalyst. However, in this specific scenario, increasing the temperature will shift the reaction to the right.