The stoichiometric equation for the oxidation of bromide ions by hydrogen peroxide in acid solution is 2Br − (aq) + H 2 O 2 (aq) + 2H + (aq) ⎯→ Br 2 ( λ ) +2H 2 O( λ )
Since the reaction does not occur in one stage, the rate equation does not correspond to this stoichiometric equation but is rate = k[H 2 O 2 ] [H + ] [Br − ].
Text Solution
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3; Both rates are 3.6 × 10 − 3 mole dm − 3 s −1 ; No effect; Decreased by a factor of 8; No effect
Sol. 2Br − (aq) + H 2 O 2 (aq) + 2H + (aq) ⎯→ Br 2 ( λ ) +2H 2 O ( λ )
rate ( nj ) = k [H 2 O 2 ] [H + ] [Br – ] = 
= 
R 1 = k [H 2 O 2 ] [H + ] [Br – ] = 3R 1
= 3R 1 = k 1 [H 2 O 2 ] [H + ] [Br – ]
= 
= 
= 
= 
= 
= 
= 
= + 
[ 7.2 × 10 –3 ] = 
= + 
3.6 × 10 –3 = 
= + 
No effect
r 1 = k [H 2 O 2 ] [H + ] [Br – ] = 
r 2 = k 
= 
r 2 = 
[k (H 2 O 2 )] [H + ] [Br – ] = 
= 
r 1 = 
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