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Faraday's First Law

The reaction ...

Question

The reaction $Z n + C u S O_{4} = C u + Z n S O_{4}$ goes completely to the right. In one experiment $10 g$ of metallic zinc was added to $200 m L$ of copper sulphate solution.

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Solution

$Z n + C u S O_{4} \to C u + Z n S O_{4}$
Mass of $Z n = 10 g$ .
Volume of $C u S O_{4} = 200 m L$
Total solid at end of reaction $= 9.810 g$
$C u$ deposited $=$ ?
$[C u S O_{4}] =$ ?
Moles of $Z n = \frac{10}{65.3} = 0.153$
Let $x$ mole $(Z n)$ react with $C u S O_{4}$
$∴$ Moles of unreacted $Z n = 0.153 - x$
$\frac{(0.153 - x) \times 65.3}{m a s s o f Z n} + \frac{63.54 x}{m a s s o f C u} = 9.81$
$x = 0.1036$
$∴$ moles of $C u = 0.1036$
(1) Mass of $C u = 0.1036 \times 63.54$
$= 6.58 g$
(2) Molarity of $C u S O_{4} = \frac{x}{200} \times 1000$
$= \frac{0.1036 \times 1000}{200}$
$= 0.518 M$

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Similar questions

Q. Zinc reacts with

{C u S O}_{4}

according to the equation,

Z n + {C u S O}_{4} \to {Z n S O}_{4} + C u

. If an excess of zinc is added to 100ml, 0.05M

{C u S O}_{4}

, the amount of copper formed in moles will be :

Q. Zinc reacts with

C u {S O}_{4}

according top the equation

Z n + C u {S O}_{4} ⟶ Z n {S O}_{4} + C u

. if excess of zinc is added to

100 m l

0.05 M

C u {S O}_{4}

the amount of copper formed is:

Q. An electrochemical cell is constructed by immersing a piece of copper wire in 50 ml of 0.1 M

C u S O_{4}

solution and zinc strip in 50 ml of 0.1 M

Z n S O_{4}

E_{C u^{+ 2} / C u}^{0}

E_{Z n^{+ 2} / Z n}^{0}

= -0.76 V ]

In a separate experiment, 50 ml of 1.4 M

N H_{3}

C u S O_{4}

solution. EMF of the cell is:

K_{f}

[C u (N H_{3})_{4}]

6 \times 10^{13}

Z n

dust is added to sufficiently large volume of aqueous solution of copper sulphate.

3.175

g of copper metal and

20

J of heat is evolved. The

Δ H

for the reaction is:

Z n (s) + C u S O_{4} (a q) ⟶ Z n S O_{4} (a q) + C u (s)

(Atomic weight of

Z n = 65.3

, atomic weight of

C u = 63.5

)

Zinc granules were added to zinc sulphate, copper sulphate, aluminium sulphate and iron sulphate solutions as shown below. You would observe the deposition of metal on zinc in beakers:

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