Question

Given :

$E^{0}(\text{Cu2+ }|\text{ Cu})\text{ = 0.337 V and }\text{E}^{0}\ (\text{S}\text{n}^{\text{2+ }}\text{Sn})\text{ = - 0.136V.}$ Which of the following statements is correct?

• A. $\text{C}\text{u}^{\text{2+}}\text{ ions can be reduced by }\text{H}_{2}(g)$
• B. Cu can be oxidized by $H^{+}$
• C. $\text{S}\text{n}^{\text{2+}}$ions can be reduced by H2(g)
• D. Cu can reduce $\text{S}\text{n}^{\text{2+}}$

Answer 1

Answer: (A)

$\text{C}\text{u}^{\text{2+}}\text{ ions can be reduced by }\text{H}_{2}(g)$

Answer 2

As ${E^{0}}_{Cu2 +}\overset{\quad\quad}{\rightarrow}Cu = 0.337V > {E^{0}}_{H + /H_{2}}\therefore$ Cu2+ can

be reduced by H2