Question: For the reaction 2Cu(s) + S(s) Cu2S(s) Ho and Go are negative and So is positive. a. At equilibrium, will reactants or products predominate?

For the reaction
2Cu(s) + S(s) → Cu2S(s)
∆Ho and ∆Go are negative and ∆So is positive.
a. At equilibrium, will reactants or products predominate? Why?
b. Why must the reaction system be heated in order to produce copper (I) sulfide?

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