Question

Consider the following reaction where Kc = 1.29x10^-2 at 600 K: CO(g) + Cl2(g) --> COCl2(g)

A reaction mixture was found to contain 5.48x10^-2 moles of CO(g), 3.74×10^-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:

1. In order to reach equilibrium COCl2(g) must be produced.

2. In order to reach equilibrium Kc must decrease.

3. In order to reach equilibrium CO must be consumed.

4. Qc is less than Kc.

5. The reaction is at equilibrium. No further reaction will occur.

Answer 1

The reaction is co (9) + C₂ (8) will The Ke of the reaction is 1.29x10-2 A reaction mature contains 5.48x 15 moles of co, 3-74 x 10-2 moles a, and ollu moles cock (8) [cock [w][₂] 5-48x10 23. Jux 20-2 0.114 OL 2 55.62 As & Like so the equilibrium should shift to the left I In order to reach equilibrium cola (8) must be produced. [FALSE If coch, is powanced then & Increases and becomes more than ke ? FALSE ke of a reaction is constant at a particular condition. So ke remains unchanged aces co must be removed from the ispustom 4 FALSE 3 FALSE that from calentation we can say de 7kc

5 FALSE The reaction is not at equilibrium and he reaction moves to the left. de >ke as