Question

The following reaction was carried out in water :
Br2 +2I^- ➡ 2Br +
+ I2
The initial concentration of I^- was 0.30 M and the concentration after 10 minutes
reduced to 0.28 M. Calculate the rate of disappearance of I^- and production of I2. ​

Answer 1

Answer:

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Answer 2

The rate of disappearance of $I^{-}$ and  production of $I{2}$ the $1*10^{-3} mol^{-1}min^{-1}$.

Explanation:

Δ$[I^{-}]=[I^{-}]_{final} -[I^{-}]_{initial}$

$=0.28-0.30$

$=-0.02 mol L^{-1}$

Δ$t$=$10-0$

$=10min$

$\frac{I^{-}}{t} =\frac{-(-0.02)}{10}$

$=0.002 mol L^{-1}min^{-1}$

Rate of appearance of $I_{2} =\frac{1}{2}$Δ/Δ$\frac{[I^{-}]}{t}$

$=\frac{0.002}{2}$

$=0.001mol^{-1}min^{1}$

$=1*10^{-3} mol^{-1}min^{-1}$.