A) Increase the E and shift equilibrium to the right
B) Lower the E and shift equilibrium to the right
C) Lower the E and shift equilibrium to the left
D) Increase the E and shift equilibrium to the left
Correct Answer: A
Solution :
\[Z{{n}_{(s)}}+2{{H}^{+}}_{(aq)}\] ? \[Zn_{(aq)}^{2+}+{{H}_{2(g)}}\] \[{{E}_{Cell}}=E_{Cell}^{0}-\frac{.059}{2}\log \frac{[Z{{n}^{2+}}]}{{{[{{H}^{+}}]}^{2}}}\] When \[{{H}_{2}}S{{O}_{4}}\]is added then \[[{{H}^{+}}]\] will increase therefore \[{{E}_{Cell}}\]will also increases and equilibrium will shift towards right.You need to login to perform this action.
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