The given reaction is as follows:
2H₂O₂(l) → 2H₂O(l) + O₂(g) ΔH = -196.1kj
The decomposition of 2 moles of hydrogen peroxide in the aforementioned reaction results in the emission of 196.1 kJ of heat.
1.88x106 kJ heat is released when 652 kg of H₂O₂ decomposes.
<h3>Solution ;</h3>
The formula to calculate moles is as follows:
Moles = Mass / Molar Mass
The molar mass of H2O2 is 34.01 g/mol.
On substituting values in formula,
Moles = 361kg
34.01g / mol =361000g / 34.01g/mol (Since,1kg=1000g) = 10,614.53mol
From the stoichiometry, 2 moles of hydrogen peroxide release 196.1 kJ of heat.
So, 10,614.53 moles of hydrogen peroxide will release 10,614.532×196.1=1.04×10^6kJ of heat.
So finally we can say that 1.88x106 kJ heat is released when 652 kg of H₂O₂ decomposes.
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