Chemistry College

Identify three specific changes that could be made to a chemical system that will shift the equilibrium to increase the yield of NH3 in the following reaction:
N2(g) + 3H2(g) → 2NH3(g) + Heat

Answers

Answer 1

Three changes could be made to a chemical system to shift the equilibrium to increase the yield of NH3 in the reaction [tex]N_{2} (g)[/tex] + [tex]3H_{2} (g)[/tex] → [tex]2NH_{3} (g)[/tex] + Heat are Increase the pressure, Decrease the temperature, and Add a catalyst.

1. Increase the pressure: According to Le Chatelier's principle, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas. In this case, that means increasing the pressure on the left-hand side of the equation, where there are only two moles of gas (one [tex]N_{2}[/tex] and three [tex]H_{2}[/tex]), compared to the two moles of gas on the right-hand side (two [tex]NH_{3}[/tex]). By increasing the pressure, more of the reactants will be forced to react and produce more [tex]NH_{3}[/tex].

2. Decrease the temperature: The forward reaction in this equation is exothermic, meaning that it releases heat. According to Le Chatelier's principle, decreasing the temperature will shift the equilibrium towards the side of the equation that produces heat. In this case, that means shifting towards the products (the right-hand side). By decreasing the temperature, more [tex]NH_{3}[/tex] will be produced.

3. Add a catalyst: Adding a catalyst can increase the rate of the reaction, which can also shift the equilibrium towards the products. In this case, a catalyst like iron can be added to the reaction to increase the rate of [tex]NH_{3}[/tex] production. This will allow more [tex]NH_{3}[/tex] to be produced in the same amount of time, effectively increasing the yield.

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Related Questions

A gas at a pressure of 2.0 atm occupies a volume of 20 liters. If the volume is decreased to 10 liters and the pressure is increased to 4.0 atm, what will be the final volume of the gas?

Answers

The initial condition of the gas can be expressed using the combined gas law:

P1V1 / T1 = P2V2 / T2

where P1 = 2.0 atm, V1 = 20 L, and T1 is the initial temperature (which we will assume remains constant).

If the volume is decreased to 10 L and the pressure is increased to 4.0 atm, the new conditions can be expressed as:

P2 = 4.0 atm, V2 = ?, and T2 = T1

We can rearrange the combined gas law to solve for V2:

V2 = (P1V1T2) / (P2T1)

Plugging in the given values, we get:

V2 = (2.0 atm x 20 L x T1) / (4.0 atm x T1) = 10 L

Therefore, the final volume of the gas is 10 liters.
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