Question

How much heat should be released when 10.00 ml of H2o2 decompose if the density is 1.0095 ? Thank you

Answer 1

Answer De composition of H₂O2 : 2 H₂O₂ (1) 2H₂0 (1) + O₂ (9) Heat of reaction, a Hoxn - 2 molx 4Hz (Hz0)e] + [1 mol X - [2 ( x 4 (H2O)1] (448= standard enthalpy) - J2m01XE285.83 kJ/mol + Imol x O KT/mor] f of formation - [2 mol x 6187.78 kJ/m01)] - - 19601 KJ so 196.1 kJ of heat are released from decomposition of a moles of H₂O₂ (1) Molar mass of H₂O2 = 34.01 g/mol . 2 moles of H₂O2 = (2x 34.01)g of H₂O2 = 68.02 g of H₂O2 10 mL of H₂O2 = (10X1.0095) g of H₂O2 Imass=(volume) - 10.095g of H₂O2 SO 68.02 g of H₂O2 release 196.1 kJ of heat upon decomposition : 10.0959 " " (density) " . (196-1 x10.095) XJ " (68.02 - 29.10 kJ of heat so 29.10 kJ/of heat will be released