The value of the reactant quotient ∅for the cell is Zns/Zn^(2+)0.01M‖Cu^(2+)1.25M/Cus

Correct answer: (C) 8×10^(-3). We know that the cell reaction will be Zn_s + Cu^(2+) → Zn^(2+) + Cu_s 1.25 M 0.01 M So the reaction Quotient from the reaction will be Q = (Zn^(2+))/(Cu^(2+))Q = 0.01/1.25Q = 8 × 10^(-3)

Q25 / 160 · TS EAMCET 2021 (04 Aug Shift 2) · Chemistry

The value of the reactant quotient $(\emptyset)$ for the cell is
$Zn (s) / {Zn}^{2 +} (0.01 M) ‖ {Cu}^{2 +} (1.25 M) / Cu (s)$

A
$1$
B
$2 \times 10^{- 2}$
Correct answer
C
$8 \times 10^{- 3}$
D
$1.25$

Solution

We know that the cell reaction will be

$\begin{matrix} {Zn}_{(s)} & + & {Cu}^{2 +} & \to & {Zn}^{2 +} & + & {Cu}_{(s)} \\ 1.25 M & 0.01 M \end{matrix}$

So the reaction Quotient from the reaction will be

$Q = \frac{[{Zn}^{2 +}]}{[{Cu}^{2 +}]} Q = \frac{0.01}{1.25} Q = 8 \times 10^{- 3}$

Hence, the correct answer is option: 'C'.

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The value of the reactant quotient ∅for the cell isZns/Zn2+0.01M‖Cu2+1.25M/Cus

Solution

Relevant Questions

The value of the reactant quotient $(\emptyset)$ for the cell is
$Zn (s) / {Zn}^{2 +} (0.01 M) ‖ {Cu}^{2 +} (1.25 M) / Cu (s)$