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
i was told right by some people and left by some people.???
You received different answers because you didn't make it clear which way the reaction is going to obtain delta H of +92.4 kJ and/or some of the responders didn't note that it is delta Ho.
delta Ho is the heat of FORMATION which means
1/2 N2 + 3/2 H2 ==> NH3 delta Ho = delta Hrxn = 46.2 kJ/mol
So for your reaction, we have
N2 + 3H2 ==> 2NH3 for which delta H rxn = +92.4 kJ.
That makes the equation I've written an endothermic reaction and adding heat will shift it to the right (to the NH3 side)
To determine the effect of increasing temperature on the given reaction, we need to consider Le Chatelier's Principle. According to Le Chatelier's Principle, an increase in temperature will favor the endothermic direction of a reaction (in this case, the forward reaction).
In the given reaction:
2NH3 (g) ↔ N2 (g) + 3H2 (g) ΔH° = +92.4 kJ
Since the forward reaction is endothermic (positive ΔH°), increasing the temperature will shift the reaction to the right, favoring the formation of N2 and H2 products.
Therefore, the answer is: d) right
To determine the effect of temperature on the equilibrium position, we need to consider Le Chatelier's principle. According to Le Chatelier's principle, when a system at equilibrium is subjected to a stress, the system responds by shifting the equilibrium position to counteract the stress.
In this case, we are increasing the temperature, which is a stress. An increase in temperature can be considered as adding energy to the system. To counteract this increase in temperature, the system will shift in the direction that consumes or absorbs heat. In other words, the reaction will move in the direction that is endothermic.
Looking at the given reaction, we can see that the forward reaction (2NH3 (g) -> N2 (g) + 3H2 (g)) is endothermic because it absorbs energy (ΔH° = +92.4 kJ). Therefore, increasing the temperature will favor the endothermic reaction and shift the equilibrium position to the right, which produces more products (N2 and H2).
Hence, the correct answer is (d) right.