Answer:
a. NO is added to the reaction mixture ⇒ to the left
b. BrNO is added to the reaction mixture ⇒ to the right
c. Br₂ is removed from the reaction mixture ⇒ to the right
d. Pressure is increased ⇒ to the left
Explanation:
The reaction at equilibrium is the following:
2BrNO (g) → 2NO (g)+ Br₂ (g)
The left side is the reactants side (2 BrNO) and the right side is the products side (2 NO + Br₂).
<em>a. </em><em>NO is added to the reaction mixture</em>
NO is a product, in the right side of the equation. If a product is added, the equilibrium will shift to the opposite side, to the left, to form more reactants and compensate for the addition.
<em>b.</em><em> BrNO is added to the reaction mixture</em>
BrNO is a reactant, in the left side of the equation. If a reactant is added to a reaction at equilibrium, more product will be formed in compensation. Therefore, the equilibrium will shift to the right.
<em>c.</em><em> Br₂ is removed from the reaction mixture</em>
Br₂ is a product, in the right side. If it is removed, the system will compensate for the remotion by forming more product, so the reaction will shift to the right.
<em>d. </em><em>Pressure is increased</em>
Since both reactants and products are in the gas phase, the equilibrium is affected by pressure. If pressure is increased, the equilibrium will shift to the side of the reaction with the fewest number of moles. The reactants side (left) has 2 moles of BrNO while the products side (right) has 3 moles (1 mol NO + 1 mol Br₂ = 3 moles of gas). Therefore, the reactants side has the fewest number of moles, so the equilibrium will shift to the left.
