Hydrogen peroxide can decompose to water and oxygen by the reaction 2H2O2(l) -> 2H2O(l) + O2(g) ?H = -196 kJ Calculate the quantity of heat released when 5.00 g of H2O2(l) decompose at constant pressure.
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The molar mass of H2O2 is approximately 34.02 g/mol. So, 5.00 g of H2O2 is about 0.147 moles. The reaction equation tells us that 2 moles of H2O2 decompose to release -196 kJ of heat. Show more…
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Hydrogen peroxide can decompose to water and oxygen by the reaction: 2 H2O2(l) → 2 H2O(l) + O2(g) ∆H = -196 kJ. Calculate the quantity of heat released when 5.00 g of H2O2(l) decomposes at constant pressure.
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Hydrogen peroxide can decompose to water and oxygen by the reaction: 2H2O2(l) ---> 2H2O(l) + O2(g) ΔH = -196 kJ Calculate the quantity of heat released when 5.00 g of H2O2(l) decomposes at constant pressure.
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Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition: $$2 \mathrm{H}_{2} \mathrm{O}_{2}(l) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g) \quad \Delta H=-196.1 \mathrm{kJ}$$ How much heat is released when 652 $\mathrm{kg}$ of $\mathrm{H}_{2} \mathrm{O}_{2}$ decomposes?
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