You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Rate Constant

The following...

Question

The following reaction was carried out in water, ${C l}_{2} + 2 I^{-} ⟶ I_{2} + 2 {C l}^{-}$ .
The initial concentration of $I^{-}$ was $0.25$ $m o l$ $L^{- 1}$ and the concentration after $10$ minutes was $0.23$ $m o l$ $L^{- 1}$ . Calculate the rate of disappearance of $I^{-}$ and appearance of $I_{2}$ .

Open in App

Solution

$Δ [I^{-}] = {[I^{-}]}_{f i n a l} - {[I^{-}]}_{i n i t i a l}$
$= 0.23 - 0.25 = - 0.02$ $m o l$ $L^{- 1}$
$Δ t = 10 - 0 = 10$ $m i n$
$- \frac{Δ [I^{-}]}{Δ t} = - \frac{(- 0.02)}{10} = 0.002$ $m o l$ $L^{- 1}$ ${m i n}^{- 1}$
Rate of appearance of $I_{2} = - \frac{1}{2} \frac{Δ [I^{-}]}{Δ t} = \frac{0.002}{2}$
$= 0.001$ $m o l$ $L^{- 1}$ ${m i n}^{- 1}$
$= 1 \times 10^{- 3}$ $m o l$ $L^{- 1}$ ${m i n}^{- 1}$

Suggest Corrections

Similar questions

{C l}_{2} + 2 I^{-} \to I_{2} + 2 {C l}^{-}

The initial concentration of

I^{-}

was

0.25 m o l

L^{- 1}

and the concentration after

10

minutes

0.23 m o l

L^{- 1}

. Calculate the rate of disappearance of

I^{-}

and appearance of

I_{2}

Q. For the reaction,

C l_{2} + 2 I^{-} \to I_{2} + 2 C l^{-}

, the initial concentration of

I^{-}

was

0.20 m o l l i t^{- 1}

and the concentration after

20

min was

0.18 m o l l i t^{- 1}

. Then, the rate of formation of

I_{2}

m o l l i t^{- 1} m i n^{- 1}

would be:

Q. Reaction:

C l_{2} (g) + 2 I^{-} (a q) \to I_{2} (g) + 2 C l^{-} (a q)

Initial concentration of

I^{- 1} = 0.30

mole

l i t r e^{- 1}

Final concentration of

I^{- 1} = 0.25

mole

l i t r e^{- 1}

after

1

minutes. Determine Rate of disappearance of

I^{- 1}

. Rate of formation of

I_{2}

Q. For the reaction

C l_{2} + 2 I^{-} \to I_{2} + 2 C l^{-}

, the initial concentration of

I^{-}

was 0.2 mol

L^{- 1}

and the concentration after 20 min was 0.18 mol

L^{- 1}

. The rate of formation of l2 in mol

L^{- 1} m i n^{- 1}

would be

Q. For the reaction,

A + B \to C

The concentration of

A

initially was observed to be

0.2 m o l / L

and the concentration of

A

after

20 m i n

was found out to be

0.16 m o l / L

.

Calculate the average rate of reaction

(r_{a v})

for first

20 m i n

m o l L^{- 1} m i n^{- 1}

Join BYJU'S Learning Program

The following reaction was carried out in water, Cl2+2I−⟶I2+2Cl−.The initial concentration of I− was 0.25 mol L−1 and the concentration after 10 minutes was 0.23 mol L−1. Calculate the rate of disappearance of I− and appearance of I2.

Δ[I−]=[I−]final−[I−]initial =0.23−0.25=−0.02 mol L−1Δt=10−0=10 min−Δ[I−]Δt=−(−0.02)10=0.002 mol L−1 min−1Rate of appearance of I2=−12Δ[I−]Δt=0.0022 =0.001 mol L−1 min−1 =1×10−3 mol L−1 min−1