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1. 1 Cu2+ (aq) + 4 Cl- (aq) ⇌ 1 [CuCl4]2–(aq) which reaction shifted the chemical...

1.

1

Cu2+ (aq) +

4

Cl- (aq) ⇌

1

[CuCl4]2–(aq)

which reaction shifted the chemical equilibrium towards the forward direction? Which reaction shifted the chemical equilibrium towards the reverse direction? Explain your reasoning for both using Le Châtelier’s principle.

2. How does the temperature affect the copper(II) chloride equilibrium? Use Le Chatelier’s principle to explain whether the forward reaction is considered an exothermic or endothermic reaction.

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Answer #1

1. Incomplete question.

2. This reaction is exothermic this is because here spontanity is decreased means DS<0 because ions bind together to form a compound. And in Gibbs energy equation DG = DH -TDS (D = Change)

Since DS <0 means TDS will be +ve and DG = 0 since equilibrium is there so to make if 0 DH must be -ve whic h signify that reaction is exothermic.

So on heating or increasing the temprature the reaction will shift towards reactant backward direction.

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