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Potassium Permanganate

Ag → 2Bg+Cg ...

Question

$A (g) \to 2 B (g) + C (g)$
$t = 0, A = 2 m o l e, B = 0, C = 0$
The total number of moles of B and C at the end of 50% reaction are:

A

2

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B

3

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C

5

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D

None

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Solution

The correct option is D 3
When 1 mole of A is present then 2 mole of B and C will forms after completion of the reaction but when 50% is complete then the total mole = $1 + 2 = 3$

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Similar questions

A (g) \to 2 B (g) + C (g)

t = 0, A= 2 mole - -
The total number of moles of A, B and C at the end of 50% reaction are:

Q. For the system

A (g) + 2 B (g) ⇌ C (g)

, the equilibrium concentration for

A, B

C

m o l e s / l i t r e

0.06, 0.12

0.216

respectively.The

K_{e q}

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Q. For the reaction

A (g) + 2 B (g) ⇌ C (g) + D (g);

K_{c} = 10^{12} v o l m e . m o l e^{- 1}

. If the initial moles of

A, B, C

D

0.5, 1, 0.5

3.5

moles respectively in a one litre vessel. The equilibrium concentration of

B

Q. For the reaction

A (g) + 2 B (g) \to C (g) + D (g); K_{c} = 10^{12}

.
If the initial moles of

A, B, C

D

0.5, 1, 0.5

3.5

moles respectively in a one litre vessel. What is the equilibrium concentration of

B

?

For the system A(g) + 2B(g) $⇌$ C(g), the equilibrium concentrations are (A)

0.06 mole/litre (B) 0.12 mole/litre (C) 0.216 mole/litre. The $K_{e q}$ for the

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