How Is Heat Released When Hydrogen Peroxide Decomposes?

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SUMMARY

The decomposition of hydrogen peroxide (H2O2) into water (H2O) and oxygen (O2) releases heat, quantified by the reaction 2H2O2 (l) = 2H2O (l) + O2 (g) with a ΔH of -196 kJ. To calculate the heat released (q) when 5.00 g of H2O2 decomposes, one must first determine the number of moles of H2O2 present. This involves using the molar mass of H2O2, which is approximately 34.01 g/mol, leading to 0.147 moles of H2O2 in 5.00 g. Consequently, the heat released can be calculated using the formula q = moles × ΔH, resulting in q = -14.4 J.

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hydrogen peroxide can decompose to water and oxygen by following reaction:
2H2 O2 (l) = 2H2 O(l) + O2(g) deltaH= -196kJ

CALCULATE THE VALUE OF q when 5.00g of H2 O2(l) decomposes at constant pressure.

my answer is -14.4J...can some please tell me how to do this again because I forgot what step I took and it have a similar question on another homework
 
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delta H is in terms of kJ per mole of equation; how many moles of H2O2 are there in 5.00g and how many 'moles of equation' are there?
 

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