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A student ran the following reaction in the laboratory at 610 K: CO(g) + Cl2(g) COCl2(g) When she...

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Chemistry

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.  

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)  

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.  

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

Answer & Explanation Solved by verified expert
4.3 Ratings (574 Votes)
Part 1Initial concentration of Cl2 0211MInitial concentration of CO 0183MCOg Cl2g    See Answer
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