CS2(g) + 3Cl2(g) CCl4(g) + S2Cl2(g)At a given temperature, the ...

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Question 1

Consider the reaction:

    CaCl₂(s) + 2H₂O(g) CaCl₂·2H₂O(s)

The equilibrium constant for the reaction as written is:

◦ K =
◦
◦
◦ K = [H₂O]²
◦ K =

Question 2

CS₂(g) + 3Cl₂(g) CCl₄(g) + S₂Cl₂(g)

At a given temperature, the reaction above is at equilibrium when [CS₂] = 0.050 M, [Cl₂] = 0.25 M, [CCl₄] = 0.15 M, and [S₂Cl₂] = 0.35 M. What would be the direction of the reaction when the reactants and products have the following concentrations: CS₂ = 0.16 M, Cl₂ = 0.20 M, CCl₄ = 0.31 M, and S₂Cl₂ = 0.29 M?

◦ To the right
◦ To the left
◦ No change
◦ Cannot predict unless we know the temperature
◦ Cannot predict unless we know whether the reaction is endothermic or exothermic

[carlsona147]

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Thanks for the timely response, appreciate it

[deja]

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