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1) A student ran the following reaction in the laboratory at 306 K: CH4(g) + CCl4(g)...

1)

A student ran the following reaction in the laboratory at 306 K:

CH4(g) + CCl4(g) 2CH2Cl2(g)

When she introduced 3.94×10-2 moles of CH4(g) and 5.52×10-2 moles of CCl4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2Cl2(g) to be 8.23×10-3 M.

Calculate the equilibrium constant, Kc, she obtained for this reaction.

Kc=

2)

A student ran the following reaction in the laboratory at 333 K:

CH4(g) + CCl4(g) 2CH2Cl2(g)

When she introduced 3.94×10-2 moles of CH4(g) and 7.17×10-2 moles of CCl4(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 6.56×10-2 M.

Calculate the equilibrium constant, Kc, she obtained for this reaction.

Kc =

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