Please tell me if these are right.

1.According to Le Chatelier’s principle, what is the effect on the products when N2 is added to the equilibrium mixture of each of the following reactions?

a. 2NH3(g) < = > 3H2(g) + N2(g)
B. N2(g) + O2(g) <= > 2NO(g)
C. 2NO2(g)< => N2(g) +2O2(g)
D. 4NH3(g) + 3O2(g) <= > 2N2(g) +6H2O(g)

A. equilibrium shifts to reactants
B. equilibrium shifts to products
C. equilibrium shifts to reactants
D. equilibrium shifts to products

2.Would increasing the volume of the equilibrium mixture of each of the following reactions cause the equilibrium to shift and if so will the shift be toward products or reactants.

a. 2NH3(g) < => 3H2(g) + N2(g)
B. N2(g) +O2(g) <= > 2NO(g)
C. 2NO2(g) <= > N2(g) + 2O2(g)
D. 4NH3(g) +3O2(g) <= > 2N2(g) + 6H2O(g)

A. equilibrium shifts to reactants
B. equilibrium shifts to products
C. equilibrium shifts to reactants
D. equilibrium shifts to products

To determine the effect on the products when N2 is added to the equilibrium mixture of each reaction, we can use Le Chatelier's principle. According to this principle, if a stress is applied to a system at equilibrium, the system will respond by shifting its equilibrium position to counteract the stress.

For the first question:

a. 2NH3(g) < = > 3H2(g) + N2(g)
When N2 is added, it increases the concentration of N2 on the right side of the reaction. To counteract this increase, the equilibrium will shift to the left, towards the reactants. Therefore, the correct answer is "equilibrium shifts to reactants."

b. N2(g) + O2(g) <= > 2NO(g)
Adding N2 to this reaction increases the concentration of N2 on the left side. The equilibrium will shift towards the product side to reduce the excess N2. Therefore, the correct answer is "equilibrium shifts to products."

c. 2NO2(g) < => N2(g) + 2O2(g)
Adding N2 increases the concentration on the right side of the reaction. The equilibrium will shift to the left, towards the reactants, to minimize the increase in N2. Therefore, the correct answer is "equilibrium shifts to reactants."

d. 4NH3(g) + 3O2(g) <= > 2N2(g) + 6H2O(g)
Adding N2 here increases its concentration on the right side. The equilibrium will shift to the left, towards the reactants, to counteract the increase of N2. Therefore, the correct answer is "equilibrium shifts to reactants."

For the second question:

a. 2NH3(g) < => 3H2(g) + N2(g)
Increasing the volume of the system decreases the pressure. According to Le Chatelier's principle, an increase in volume will cause the equilibrium to shift towards the side with more moles of gas to counteract the decrease in pressure. In this case, the equilibrium has 1 mole of gas on the left side and 4 moles of gas on the right side. Therefore, the equilibrium will shift towards the product side. The correct answer is "equilibrium shifts to products."

b. N2(g) + O2(g) <= > 2NO(g)
Increasing the volume will decrease the pressure, and since there are equal numbers of moles of gas on both sides of the equation, the equilibrium will not shift in any particular direction. The correct answer is "no shift in equilibrium."

c. 2NO2(g) <= > N2(g) + 2O2(g)
Increasing the volume will decrease the pressure. There are equal numbers of moles of gas on both sides of the equation, so the equilibrium will not shift in any particular direction. The correct answer is "no shift in equilibrium."

d. 4NH3(g) + 3O2(g) <= > 2N2(g) + 6H2O(g)
Increasing the volume will decrease the pressure. The left side of the reaction has 7 moles of gas, while the right side has 8 moles of gas. Therefore, the equilibrium will shift towards the side with more moles of gas, which is the right side. The correct answer is "equilibrium shifts to products."

Remember, these answers are based on the application of Le Chatelier's principle. It's important to understand the principle and how to apply it to different reactions.

1. According to Le Chatelier’s principle, the effect on the products when N2 is added to the equilibrium mixture of each of the following reactions is:

a. 2NH3(g) <=> 3H2(g) + N2(g)
The equilibrium will shift to the reactants.

b. N2(g) + O2(g) <=> 2NO(g)
The equilibrium will shift to the products.

c. 2NO2(g) <=> N2(g) + 2O2(g)
The equilibrium will shift to the reactants.

d. 4NH3(g) + 3O2(g) <=> 2N2(g) + 6H2O(g)
The equilibrium will shift to the products.

2. Increasing the volume of the equilibrium mixture of each of the following reactions will cause the equilibrium to shift, and the shift will be towards:

a. 2NH3(g) <=> 3H2(g) + N2(g)
The equilibrium will shift to the reactants.

b. N2(g) + O2(g) <=> 2NO(g)
There will be no shift in the equilibrium as there are equal numbers of moles on both sides of the reaction.

c. 2NO2(g) <=> N2(g) + 2O2(g)
The equilibrium will shift to the reactants.

d. 4NH3(g) + 3O2(g) <=> 2N2(g) + 6H2O(g)
The equilibrium will shift to the products.