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Consider the following reaction:

$$\textrm{Zn} (s) + \textrm{SnCl}_2 (aq) \rightarrow \textrm{ZnCl}_2 (aq) + \textrm{Sn} (s) \qquad E˚ = +0.60 \textrm{ V}$$

Given all of the reactants and products are at standard concentrations ($1.0 \textrm{ M}$), which of the following statements must be true?

Select ALL that apply.

A

The reaction would be spontaneous.

B

$\Delta G°$ for the reaction as written is positive.

C

An increase in the concentration of $\textrm{SnCl}_2$ would push the equilibrium towards the right.

D

An increase in the amount of $\textrm{Sn}(s)$ would push the equilibrium towards the left.

E

None of the above.

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