Multiple Choice
CS2(g) + 3Cl2(g) ![CS<sub>2</sub>(g) + 3Cl<sub>2</sub>(g) CCl<sub>4</sub>(g) + S<sub>2</sub>Cl<sub>2</sub>(g) At a given temperature,the reaction above is at equilibrium when [CS<sub>2</sub>] = 0.050 M,[Cl<sub>2</sub>] = 0.25 M,[CCl<sub>4</sub>] = 0.15 M,and [S<sub>2</sub>Cl<sub>2</sub>] = 0.35 M.What will be the direction of the reaction when the reactants and products have the following concentrations: CS<sub>2</sub> = 0.14 M,Cl<sub>2</sub> = 0.20 M,CCl<sub>4</sub> = 0.28 M,and S<sub>2</sub>Cl<sub>2</sub> = 0.28 M? A) to the left B) to the right C) no change D) cannot predict unless we know the temperature E) cannot predict unless we know whether the reaction is endothermic or exothermic](https://d2lvgg3v3hfg70.cloudfront.net/TB2288/11ea7a3a_9f19_a09e_a82d_05e13d793f7a_TB2288_11.jpg)
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 will be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.14 M,Cl2 = 0.20 M,CCl4 = 0.28 M,and S2Cl2 = 0.28 M?
A) to the left
B) to the right
C) no change
D) cannot predict unless we know the temperature
E) cannot predict unless we know whether the reaction is endothermic or exothermic
Correct Answer:
Verified
Correct Answer:
Verified
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