$1000 \, mL$ of $1 \, M$ $CuSO_{4(aq)}$ is electrolysed by $9.65 \, A$ current for $100 \, s$ using $Pt$ electrodes. Which statement is incorrect?

Plotting $1 / \Lambda_{m}$ against $c \Lambda_{m}$ for aqueous solutions of a monobasic weak acid $(HX)$ resulted in a straight line with $y$-axis intercept of $P$ and slope of $S$. The ratio $P / S$ is
$[\Lambda_{m} =$ molar conductivity
$\Lambda_{m}^{\circ} =$ limiting molar conductivity
$c =$ molar concentration
$K_{a} =$ dissociation constant of $HX$ ]

Tollen's reagent is used for the detection of aldehyde. When a solution of $AgNO_3$ is added to glucose with $NH_4OH$,gluconic acid is formed.
$Ag^{+} + e^{-} \rightarrow Ag ; E^{\circ}_{red} = 0.8 \ V$
$C_6H_{12}O_6 + H_2O \rightarrow C_6H_{12}O_7 + 2H^{+} + 2e^{-} ; E^{\circ}_{oxd} = -0.05 \ V$
$Ag(NH_3)_2^{+} + e^{-} \rightarrow Ag_{(s)} + 2NH_3 ; E^{\circ}_{red} = 0.337 \ V$
[Use $2.303 \times \frac{RT}{F} = 0.0592$ and $\frac{F}{RT} = 38.92$ at $298 \ K$]
$1.$ $2Ag^{+} + C_6H_{12}O_6 + H_2O \rightarrow 2Ag_{(s)} + C_6H_{12}O_7 + 2H^{+}$. Find $\ln K$ of this reaction.
$(A) \ 66.13 \quad (B) \ 58.38 \quad (C) \ 28.30 \quad (D) \ 46.29$
$2.$ When ammonia is added to the solution,$pH$ is raised to $11$. Which half-cell reaction is affected by $pH$ and by how much?
$(A) E_{oxd}$ will increase by a factor of $0.65 \ V$ from $E^{\circ}_{oxd}$
$(B) E_{oxd}$ will decrease by a factor of $0.65 \ V$ from $E^{\circ}_{oxd}$
$(C) E_{red}$ will increase by a factor of $0.65 \ V$ from $E^{\circ}_{red}$
$(D) E_{red}$ will decrease by a factor of $0.65 \ V$ from $E^{\circ}_{red}$
$3.$ Ammonia is always added in this reaction. Which of the following must be incorrect?
$(A) NH_3$ combines with $Ag^{+}$ to form a complex.
$(B) Ag(NH_3)_2^{+}$ is a stronger oxidising reagent than $Ag^{+}$.
$(C)$ In absence of $NH_3$,silver salt of gluconic acid is formed.
$(D) NH_3$ has affected the standard reduction potential of glucose/gluconic acid electrode.
Give the answer for questions $1, 2$ and $3$.

Calculate the standard cell potentials of galvanic cells in which the following reactions take place:
$(i)$ $2Cr_{(s)} + 3Cd^{2+}_{(aq)} \rightarrow 2Cr^{3+}_{(aq)} + 3Cd_{(s)}$
$(ii)$ $Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} \rightarrow Fe^{3+}_{(aq)} + Ag_{(s)}$
Calculate the $\Delta_r G^\Theta$ and equilibrium constant of the reactions.

For the fuel cell reaction:
$2H_{2(g)} + O_{2(g)} \to 2H_2O_{(l)}$; $\Delta_fH^o_{298}(H_2O_{(l)}) = -285.5 \ kJ/mol$
What is $\Delta S^o_{298}$ for the given fuel cell reaction?
Given: $O_{2(g)} + 4H^+_{(aq)} + 4e^- \to 2H_2O_{(l)}$; $E^o = 1.23 \ V$

On the basis of standard electrode potential values,suggest which of the following reactions would take place?