Hydrogen peroxide can decompose to water and oxygen according to: 2H 2 O 2 (l) +

Question

Hydrogen peroxide can decompose to water and oxygen according to:

2H2O2(l) + -----------> 2H2O (l) + O2(g) ^ H = -196 kJ

What is the enthalpy change accompanying the reaction of 5.00 g H2O2(l) according to the above mentioned reaction ?

Explanation / Answer

Hydrogen peroxide can decompose to water and oxygen according to: 2H2O2(l) + -----------> 2H2O (l) + O2(g) ^ H = -196 kJ What is the enthalpy change accompanying the reaction of 5.00 g H2O2(l) according to the above mentioned reaction ? ANSWER: 2H2O2(l) + -----------> 2H2O (l) + O2(g) Delta H = -196 kJ Step 1: Convert moles. 5.00 g/34.01 g/mol = 0.147 mole H2O2. Step 2: According to the equation, 2 mole H2O2 produce -196 KJ. 0.147 mole H2O2 x(-196 KJ/2 moles H2O2) = -14.41 KJ So 5 g H2O2 produce the enthalpy (delta H) change is -14.41 KJ.

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