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Reaction with Metals

MnO2 + 2KClO3...

Question

$M n O_{2} + 2 K C l O_{3} ⟶ K_{2} M n O_{4} + C l_{2} + 2 O_{2}$
$C l_{2} + K M n O_{4} ⟶ 2 K C l + M n O_{2} + O_{2}$
Each reaction takes place to the extent of $50 %$ . $11.2$ L of $O_{2}$ at STP is obtained from $K C l O_{3}$ using :

4

mol

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1.12

mol

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1.33

mol

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2.66

mol

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Solution

The correct option is A $4$ mol
$M n O_{2} + 2 K C l O_{3} ⟶ K_{2} M n O_{4} + C l_{2} + 2 O_{2}$
$C l_{2} + K M n O_{4} ⟶ 2 K C l + M n O_{2} + O_{2}$
According to the balanced reaction,
$11.2$ L $O_{2}$ ( $0.5$ mole) = $1$ mole $C l_{2} = 4$ moles $K C l O_{3}$
$50 %$ yield $50 %$ yield

Suggest Corrections

Similar questions

M n O_{2} + 2 K C l O_{3} \to K_{2} M n O_{4} + C l_{2} + 2 O_{2}

C l_{2} + K_{2} M n O_{4} \to 2 K C l + M n O_{2} + O_{2}

O_{2}

K C l O_{3}

M n O_{2} + 2 K C l O_{3} ⟶ K_{2} M n O_{4} + C l_{2} + 2 O_{2}

C l_{2} + K M n O_{4} ⟶ 2 K C l + M n O_{2} + O_{2}

50 %

11.2

O_{2}

K C l O_{3}

5.0

K C l O_{3}

0.03

O_{2}

K C l O_{3}

2 K C l O_{3} ⟶ 2 K C l + 3 O_{2}

M n O_{2} + 4 H C l \to 2 H_{2} O + M n {C l}_{2} + {C l}_{2}

M n O_{2}

H C l

2.24 L

{C l}_{2}

M n O_{2}

M n = 55 g / m o l

M n O_{2} + 4 H C l ⟶ M n C l_{2} + 2 H_{2} O + C l_{2}

2

M n O_{2}

4

H C l

11.2

C l_{2}

C l_{2}

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