SalenaGallagher84
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Given the reaction at equilibrium:
N2(g) + 3H2(g) -->2NH3(g) + 91.8 kJ
What occurs when the concentration of H2(g) is increased?
(1) The rate of the forward reaction increases and the concentration of N2(g) decreases.
(2) The rate of the forward reaction decreases and the concentration of N2(g) increases.
(3) The rate of the forward reaction and the concentration of N2(g) both increase.
(4) The rate of the forward reaction and the concentration of N2(g) both decrease.



Answer :

(1) The rate of the forward reaction increases and the concentration of N2(g) decreases.
N2 is constant 
Oseni

If the concentration of [tex]H_2 (g)[/tex] is increased, the rate of the forward reaction increases and the concentration of [tex]N_2 (g)[/tex] decreases.

Le Chartelier principle

The principle states that reactions in equilibrium being disturbed by factors such as temperature, the concentration of species in the reaction, etc, will experience a shift in the equilibrium so as to annul the effects of the disturbance.

Thus, adding more of the reactants ( [tex]H_2 (g)[/tex] to the reaction will see more  products being synthesized. This means more  [tex]N_2 (g)[/tex] will be consumed and its concentration will decrease accordingly.

More on Le chartelier principle can be found here: https://brainly.com/question/12099569

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