n2 g 3h2 g 2nh3 g + 22,000 cal Explain how the equilibrium is shifted when more nitrogen is added?

Sam. You must learn to write equation correctly. n2 g I must guess what that means. No arrow. I must guess what are reactants and what are products. However, I can tell you that if more nitrogen is added, the reaction will shift is such a way as to use up the nitrogen. Which way is that?

to the right which is 2NH3 g

To explain how the equilibrium is shifted when more nitrogen is added in the given chemical equation, we need to understand Le Chatelier's principle. According to this principle, if a system at equilibrium is subjected to a change, it will respond by shifting its equilibrium position to counteract that change.

In this equation, the reactants are nitrogen gas (N2) and hydrogen gas (H2), which react to form ammonia gas (NH3). The equation states that the reaction is exothermic, releasing 22,000 calories (cal) of heat.

Let's now consider the effect of adding more nitrogen gas (N2) to the reaction. By increasing the concentration of nitrogen gas, we disturb the balance of the system. In response to this change, the equilibrium will shift in a direction that consumes some of the added nitrogen in order to restore the equilibrium.

In this case, since the equation shows that the forward reaction from N2 to NH3 consumes nitrogen gas, adding more N2 will cause the reaction to shift to the right to form more NH3. By increasing the concentration of NH3, the system counteracts the addition of nitrogen gas.

To summarize, adding more nitrogen gas to the reaction will cause the equilibrium to shift to the right, favoring the formation of ammonia gas (NH3), in order to restore the balance.