Question

23. 2NO(g) + O2(g) → 2NO2(g)

How could the forward reaction be increased (how could you make more product when
getting back to equilibrium)?
a. Reduce the pressure
b. Increase the volume of the container
c. Remove some NO2(g)
d. Increase the temperature

Answer 1

To increase the amount of product NO2(g) and shift the equilibrium position right, we can:

c. Remove some NO2(g)

This will drive the equilibrium right to produce more NO2(g) according to Le Chatelier's principle.

The other options will not have the desired effect:

a. Reducing pressure will not impact the equilibrium position.

b. Increasing volume will slightly favor the forward reaction but the effect will be small.

d. Increasing temperature can either drive the equilibrium right or left depending on where the equilibrium currently lies. Without knowing the initial conditions, we cannot determine the effect.

So the correct choice is c. Remove some NO2(g). This is a common technique used industrially to maximize product yield, known as Le Chatelier's equilibrium shift.

Let me know if you have any other questions!

Answer 2

Step-by-step explanation:

d. Increase the temperature. According to Le Chatelier's principle, increasing the temperature of an endothermic reaction shifts the equilibrium towards the products to absorb the excess heat. In this case, the forward reaction is endothermic, as it requires energy to form NO2 from NO and O2. Therefore, increasing the temperature will favor the forward reaction and increase the amount of product formed.