Question

Consider the following reaction where Kc = 77.5 at 600 K: CO(g) + Cl2(g) COCl2(g) A reaction mixture was found to contain 4.24×10-2 moles of CO(g), 4.48×10-2 moles of Cl2(g) and 0.114 moles of COCl2(g), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: T 1. In order to reach equilibrium COCl2(g) must be produced. T 2. In order to reach equilibrium Kc must decrease. T 3. In order to reach equilibrium CO must be produced. F 4. Qc is greater than Kc. F 5. The reaction is at equilibrium. No further reaction will occur.

Answer 1

Answer:

The reaction mentioned in the question is:  

CO (g) + Cl₂ (g) ⇔ COCl₂ (g), the equilibrium constant or Kc will be 77.5 at 600 K. In the given mixture, the moles of CO given is 4.24 × 10⁻² moles, the moles of Cl₂ given is 4.48 × 10⁻² moles, and the moles of COCl₂ given is 0.114 moles. The volume of the container is 1.00 L.  

The concentration or Molarity can be determined by using the formula, concentration (M) = mole/volume (L),  

The molarity of CO = 4.24 × 10⁻² moles / 1.00 L = 4.24 × 10⁻² M

The molarity of Cl₂ = 4.48 × 10⁻² moles / 1.00 L = 4.48 10⁻² M

The molarity of COCl₂ = 0.114 moles / 1.00 L = 0.114 M

The reaction quotient or Qc,  

Qc = [COCl2]/[CO][Cl2]  

Qc = 0.114 / 4.24 × 10⁻² × 4.48 × 10⁻²

Qc = 60.03

Thus, Qc is less than Kc. Hence, the reaction will proceed in forward direction so that equilibrium can be attained, that is, until Qc becomes equal to Kc.  

Therefore, the product (COCl₂) will be produced, and the reactants CO and Cl₂ will get consumed.  

1. The given statement is true.  

2. The given statement is true.  

3. The given statement is false. In order to reach equilibrium, the reactants must be consumed.  

4. The given statement is true.  

5. The given statement is false, that is Qc is not equal to Kc.