A student ran the following reaction in the laboratory at 610K:
CO(g) + Cl2(g) COCl2(g)
When she introduced 0.183 moles of CO(g) and 0.211 moles of Cl2(g)into a 1.00 liter container, she found the equilibriumconcentration of Cl2(g) to be 6.72×10-2 M. Â
Calculate the equilibrium constant, Kc, she obtained for thisreaction.
2.A student ran the following reaction in the laboratory at 546K:
COCl2(g) CO(g) + Cl2(g)Â Â
When she introduced 0.854 moles of COCl2(g) into a 1.00 litercontainer, she found the equilibrium concentration of COCl2(g) tobe 0.817 M. Â
Calculate the equilibrium constant, Kc, she obtained for thisreaction.
3. Consider the following reaction:
COCl2(g) CO(g) + Cl2(g)
If 6.56×10-3 moles of COCl2, 0.377 moles of CO, and 0.372 moles ofCl2 are at equilibrium in a 16.9 L container at 772 K, the value ofthe equilibrium constant, Kp, is
