Dear student, H2O2 → H2O + 1/2 O2 Rate constant fo the first order reaction is : k = 1tlna0atk = 150ln0 50 125k = 150ln 4 min-1 rate of disappearance of H2O2 = rate of appearance of O21/2rO2 = 12 rH2O2 = 12k [H2O2] = 12×150× ln 4 × 0 05 = 6 9 × 10-4M min-1 Regards

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Solve this: () kJ/mol Decomposition of H202 follows a first order reaction. In fifty minutes the concentration of H202decrease from 0.5 to O. 125 M in one such decomposition. When the concentration of H202 reaches 0.05 M, rate of formation of 02 will be • x 10-2 mol min-l (3 6.93 x 10-4 mol min-l WEE Main-201 (2) 6.93 x 10-2 mol mirvl (4) 2.66 L at STP 77

Dear student,

H_{2} O_{2} \to H_{2} O + 1 / 2 O_{2}

Rate constant fo the first order reaction is :

k = \frac{1}{t} \ln (\frac{a_{0}}{a_{t}}) k = \frac{1}{50} l n (\frac{0.5}{_{0.125}}) k = \frac{1}{50} l n (4) m i n^{- 1}

r a t e o f d i s a p p e a r a n c e o f H_{2} O_{2} = \frac{r a t e o f a p p e a r a n c e o f O_{2}}{1 / 2} r_{O_{2}} = \frac{1}{2} r_{H_{2} O_{2}} = \frac{1}{2} k [H_{2} O_{2}] = \frac{1}{2} \times \frac{1}{50} \times \ln 4 \times 0.05 = 6.9 \times 10^{- 4} M m i n^{- 1}

Regards

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