Hydrogen peroxides decomposes in aqueous solution, into water and oxygen gas, with the rate constant 7.5 × 1 0 − 4 sec − 1 . What amount of heat is initially liberated per second , (in J) from 2.0 L o

Question

Hydrogen peroxides decomposes in aqueous solution, into water and oxygen gas, with the rate constant $7.5 \times 1 0^{- 4} sec^{- 1}$ . What amount of heat is initially liberated per second , (in J) from 2.0 L of $1.5 M - H_{2} O_{2}$ solution?

$H_{2} O_{2} (a q) \to H_{2} O (l) + \frac{1}{2} O_{2} (g)$ ; $Δ H = - 100 k J / m o l$

TestHub · Accepted Answer

Rate of reaction = k [ H 2 ​ O 2 ​ ] . Heat liberated = Rate × Volume × ∣Δ H ∣ . 7.5 × 1 0 − 4 × 1.5 × 2.0 × 100 × 1000 = 225 J.

Chemistry - Chemical Kinetics Question with Solution | TestHub

Doubts & Discussion