Which of the following statements is correct | vedclass

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(D) The Nernst equation for the given cell reaction is: $E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{n} \log \frac{[Cd^{2+}]}{[Cu^{2+}]}$.Here,the num

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less than $E^{\circ}_{cell}$ by $0.0296 \ V$

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(D) The Nernst equation for the given cell reaction is: $E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{n} \log \frac{[Cd^{2+}]}{[Cu^{2+}]}$.Here,the number of electrons transferred $n = 2$.Given that $[Cd^{2+}] = 10 [Cu^{2+}]$,so the ratio $\frac{[Cd^{2+}]}{[Cu^{2+}]} = 10$.Substituting these values into the equation: $E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{2} \log(10)$.Since $\log(10) = 1$,we get $E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{2} 	imes 1$.$E_{cell} = E^{\circ}_{cell} - 0.02955 \ V \approx E^{\circ}_{cell} - 0.0296 \ V$.Therefore,the $emf$ of the cell is less than $E^{\circ}_{cell}$ by $0.0296 \ V$.

Which of the following statements is correct regarding the $emf$ of the cell for the cell reaction,$Cd_{(s)} + Cu^{2+}_{(aq)} \longrightarrow Cd^{2+}_{(aq)} + Cu_{(s)}$,if the concentration of $Cd^{2+}$ is $10$ times greater than the concentration of $Cu^{2+}_{(aq)}$ at $298 \ K$?

Similar Questions

In which of the following Galvanic cells is the $emf$ maximum? (Given: $E_{Mg^{2+} \mid Mg}^0 = -2.36 \ V$ and $E_{Cl_2 \mid 2 Cl^{-}}^0 = +1.36 \ V$)

The $emf$ of a $Daniel$ cell at $298 \ K$ is ${E_1}$ for the cell reaction $Zn|ZnSO_4(0.01 \ M)||CuSO_4(1.0 \ M)|Cu$. When the concentration of $ZnSO_4$ is $1.0 \ M$ and that of $CuSO_4$ is $0.01 \ M$,the $emf$ changes to ${E_2}$. What is the relationship between ${E_1}$ and ${E_2}$?

Identify the correct statement$(s)$:

The reduction potential of a hydrogen half-cell will be negative if:

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