1. Tardigrade
  2. Question
  3. Chemistry
  4. Hydrogen peroxides decomposes in aqueous solution, into water and oxygen gas, with the rate constant 7.5 × 10-4 sec -1. What amount of heat is initially liberated per second, (in J ) from 2.0L of 1.5 M - H 2 O 2 solution? H 2 O 2( aq ) arrow H 2 O ( l )+(1/2) O 2 Δ H =100 kJ / mol

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Q. Hydrogen peroxides decomposes in aqueous solution, into water and oxygen gas, with the rate constant $7.5 \times$ $10^{-4} \sec ^{-1}$. What amount of heat is initially liberated per second, (in $J$ ) from 2.0L of $1.5 M - H _{2} O _{2}$ solution?
$H _{2} O _{2}( aq ) \rightarrow H _{2} O ( l )+\frac{1}{2} O _{2} \quad \Delta H =100\, kJ / mol$

Chemical Kinetics

Solution:

$H _{2} O _{2}( l ) \longrightarrow H _{2} O ( l )+\frac{1}{2} O _{2}( g )$
Rate $=7.5 \times 10^{-4} \times 1.5=11.25 \times 2 \times 10^{-4}$ mole $L ^{-1} \sec ^{-1}$
Moles decompare from $2\, L$ will be $=11.25 \times 2 \times 10^{-4}$
$=22.5 \times 10^{-4}$ mole $\sec ^{-1}$
Enerov released will be $=22.5 \times 10^{-4} \times 10^{5}=225$