Identify the correct statement(s) about the following Galvanic cell

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The net cell reaction is given as $Z n (s) + 2 A g^{+} (a q) \to_{}^{} Z n^{2 +} (a q) + 2 A g (s)$

If the salt bridge contains the salt $K C l$ , then it releases $C l^{-}$ ions into anodic solution side and $K^{+}$ ions into cathodic solution side

If the cell EMF is positive, it implies that Zn is a stronger reducing agent than Ag

If $E^{o}$ values of anode and cathode are -0.76V and $+ 0.80 V$ respectively, then $E_{c e l l}^{o} = 0.04 V$

answer is A, C, D.

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Detailed Solution

A)The net cell reaction is $Z n + 2 A g^{+} \to_{}^{} Z n^{2 +} 2 A g$
B) $E_{c e l l}^{o} = E_{C}^{o} - E_{A}^{o} = 0.80 - (- 0.76) = 1.56 V$
C)salt bridge releases cations into cathode and anions into anode solutions to maintain electrical neutrality
D) The stronger reducing agent (metal) will have lower SRP and acts as anode