The redox reaction is as follows- Cu2S -KMnO4 - H2SO4 - CuSO4 - MnSO4 - K2SO4 - H2OHow many moles of KMnO4 is reduced by 1 mole of Cu2S-

The correct option is A TwoThe unbalanced redox reaction is Cu_2S +KMnO_4 + H_2SO_4 → CuSO_4 + MnSO_4 + K_2SO_4 + H_2O .The balanced chemical equation is ...

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Standard X

Chemistry

Electrolytic Refining of Copper

The redox rea...

Question

The redox reaction is as follows:
$C u_{2} S + K M n O_{4} + H_{2} S O_{4} \to C u S O_{4} + M n S O_{4} + K_{2} S O_{4} + H_{2} O$
How many moles of $K M n O_{4}$ is reduced by 1 mole of $C u_{2} S$ ?

Two

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Four

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Three

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None of these

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Solution

The correct option is A Two
The unbalanced redox reaction is $C u_{2} S + K M n O_{4} + H_{2} S O_{4} \to C u S O_{4} + M n S O_{4} + K_{2} S O_{4} + H_{2} O$ .
The balanced chemical equation is as follows:
$C u_{2} S + 2 K M n O_{4} + 4 H_{2} S O_{4} \to 2 C u S O_{4} + 2 M n S O_{4} + K_{2} S O_{4} + 4 H_{2} O$
Thus, 1 mole of $C u_{2} S$ reduces two moles of $K M n O_{4}$ .

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Similar questions

Q. Find the number of moles of

K M n O_{4}

needed to oxidise one mole

C u_{2} S

in acidic medium. The reaction is

K M n O_{4} + C u_{2} S \to M n^{2 +} + C u^{2 +} + S O_{2}

Q. Identify the correctly balanced redox reaction using ion-electron method.

F e S O_{4} + K M n O_{4} + H_{2} S O_{4} \to F e_{2} (S O_{4})_{3} + M n S O_{4} + H_{2} O + K_{2} S O_{4}

Q. Find the number of moles of

K M n O_{4}

needed to oxidise one mole

C u_{2} S

in acidic medium. The reaction is

K M n O_{4} + C u_{2} S \to M n^{2 +} + C u^{2 +} + S O_{2}

Balance the following reaction.

F e C_{2} O_{4} + K M n O_{4} + H_{2} S O_{4} \to F e_{2} (S O_{4})_{3} + C O_{2} + M n S O_{4} + K_{2} S O_{4} + H_{2} O

Q. Balance the equation :

K M n O_{4} + H 2 S O_{4} + F e S O 4 \to K 2 S O_{4} + M n S O_{4} + F e_{2} (S O_{4})_{3} + H_{2} O

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The redox reaction is as follows:Cu2S+KMnO4+H2SO4→CuSO4+MnSO4+K2SO4+H2OHow many moles of KMnO4 is reduced by 1 mole of Cu2S?

The correct option is A TwoThe unbalanced redox reaction is Cu2S+KMnO4+H2SO4→CuSO4+MnSO4+K2SO4+H2O.The balanced chemical equation is as follows:Cu2S+2KMnO4+4H2SO4→2CuSO4+2MnSO4+K2SO4+4H2O Thus, 1 mole of Cu2S reduces two moles of KMnO4.

The redox reaction is as follows:
$C u_{2} S + K M n O_{4} + H_{2} S O_{4} \to C u S O_{4} + M n S O_{4} + K_{2} S O_{4} + H_{2} O$
How many moles of $K M n O_{4}$ is reduced by 1 mole of $C u_{2} S$ ?