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

Question

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 (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

H 2 O 2( l ) longrightarrow H 2 O ( l )+(1/2) O 2( g ) Rate =7.5 × 10-4 × 1.5=11.25 × 2 × 10-4 mole L -1 sec -1 Moles decompare from 2 L will be =11.25 × 2 × 10-4 =22.5 × 10-4 mole sec -1 Enerov released will be =22.5 × 10-4 × 105=225

Q. Hydrogen peroxides decomposes in aqueous solution, into water and oxygen gas, with the rate constant 7.5× 10−4sec−1. What amount of heat is initially liberated per second, (in J ) from 2.0L of 1.5M−H2​O2​ solution? H2​O2​(aq)→H2​O(l)+21​O2​ΔH=100kJ/mol

H2​O2​(l)⟶H2​O(l)+21​O2​(g) Rate =7.5×10−4×1.5=11.25×2×10−4 mole L−1sec−1 Moles decompare from 2L will be =11.25×2×10−4 =22.5×10−4 mole sec−1 Enerov released will be =22.5×10−4×105=225