Consider the reaction: 2N2O(g) ⇌ O2(g) + 2N2(g). Which of the following will cause a shift in the equilibrium to the right? 1. Add more N2O 2. Remove O2 3. Remove N2

1. Add N2O and

3. Remove N2

Explanation:

In equilibrium, there is a balance between the concentrations of the reactants and products. If more reactants are added, the equilibrium will shift to the right, favoring the forward reaction. This cause an increase in the concentration of the product and the equilibrium constant is unchanged.

Products can also be removed in order to increase the amount of products formed, forward reaction. This shifts the equilibrium to the right.

In the reaction 2N2O <> O2 + 2N2, adding N2O to the mixture favors the forward reaction and more products are formed, equilibrium shifts to the right.

Also, removing the product formed favors the forward reaction as more products will be formed in order to achieve equilibrium. The equilibrium therefore shifts to the right.

h let me think

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2