For the galvanic cell,Zn_{(s)} + Cu^{2+}(0.02 | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) The cell reaction is: $Zn_{(s)} + Cu^{2+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + Cu_{(s)}$Standard cell potential $E_{cell}^{0} = E_{cathode}^{0} - E

Vedclass · Accepted Answer

$109$

Vedclass · Answer

(B) The cell reaction is: $Zn_{(s)} + Cu^{2+}_{(aq)} ightarrow Zn^{2+}_{(aq)} + Cu_{(s)}$Standard cell potential $E_{cell}^{0} = E_{cathode}^{0} - E_{anode}^{0} = 0.34 \ V - (-0.76 \ V) = 1.10 \ V$Using the Nernst equation at $298 \ K$:$E_{cell} = E_{cell}^{0} - \frac{0.059}{n} \log \frac{[Zn^{2+}]}{[Cu^{2+}]}$Here,$n = 2$,$[Zn^{2+}] = 0.04 \ M$,and $[Cu^{2+}] = 0.02 \ M$$E_{cell} = 1.10 - \frac{0.059}{2} \log \frac{0.04}{0.02}$$E_{cell} = 1.10 - 0.0295 	imes \log(2)$$E_{cell} = 1.10 - 0.0295 	imes 0.3010 \approx 1.10 - 0.00888 = 1.09112 \ V$$E_{cell} = 109.112 	imes 10^{-2} \ V$Rounding to the nearest integer,we get $109$.

For the galvanic cell,
$Zn_{(s)} + Cu^{2+}(0.02 \ M) \rightarrow Zn^{2+}(0.04 \ M) + Cu_{(s)}$
$E_{cell} = ...... \times 10^{-2} \ V \text{ (Nearest integer) }$
$[\text{Use}: E_{Cu^{2+}/Cu}^{0} = 0.34 \ V, E_{Zn^{2+}/Zn}^{0} = -0.76 \ V]$
$[\frac{2.303 \ RT}{F} = 0.059 \ V]$

Similar Questions

Fill in the blanks :
$1.$ The ratio of concentration of products to concentration of reactants is ........
$2.$ $\ln(\log(x)) =$ ............
$3.$ At equilibrium,between $E_{cell}$ and $E_{cell}^{o}$,......... will be zero.

Which of the following will increase the voltage of the cell represented by the equation
$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$

Which one of the following will increase the voltage of the cell? $(T = 298 \ K)$ :- $Sn_{(s)} + 2Ag_{(aq)}^{+} \rightarrow Sn_{(aq)}^{2+} + 2Ag_{(s)}$

If $E^{\circ}(Al_{(aq)}^{+3} \mid Al_{(s)}) = -1.66 \ V$. What is the potential of $Al_{(s)} \rightarrow Al_{(aq)}^{+3}(0.1 \ M) + 3e^-$ at $298 \ K$?

Consider the cell whose $emf$ is $1.01 \ V$.
$Pt, H_2(1 \ atm) | H^{+}(pH = 4) || Ag^{+}(xM) | Ag$
What is the value of $x$? (Given: $E^o_{Ag^{+}|Ag} = +0.8 \ V$,$\frac{2.303 \ RT}{F} = 0.06$)

Vedclass Test Series

Exam Paper Generator

Online Exam Module

For the galvanic cell,$Zn_{(s)} + Cu^{2+}(0.02 \ M) \rightarrow Zn^{2+}(0.04 \ M) + Cu_{(s)}$$E_{cell} = ...... \times 10^{-2} \ V \text{ (Nearest integer) }$$[\text{Use}: E_{Cu^{2+}/Cu}^{0} = 0.34 \ V, E_{Zn^{2+}/Zn}^{0} = -0.76 \ V]$$[\frac{2.303 \ RT}{F} = 0.059 \ V]$