Question

Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition:

2 H₂O₂(l) → 2 H₂O(l) + O₂(g) ΔHrxn = −196.1 kJ
Calculate the heat for the decomposition of 432 kg of H₂O₂.

Answer 1

To calculate the heat for the decomposition of 432 kg of H₂O₂, you can use the given equation and the enthalpy change for the decomposition of 1 mole of H₂O₂.

Step-by-step explanation:

The heat for the decomposition of 432 kg of H₂O₂ can be calculated using the given equation and the enthalpy change for the decomposition of 1 mole of H₂O₂. From the equation, we can see that 2 moles of H₂O₂ decompose to produce 1 mole of O₂. The enthalpy change for the decomposition of 1 mole of H₂O₂ is -196.1 kJ. We can use these values to calculate the heat for the decomposition of 432 kg of H₂O₂ as follows:

1. Calculate the number of moles of H₂O₂ in 432 kg using its molar mass (34 g/mol).
2. Use the mole ratio from the balanced equation to find the number of moles of O₂ produced.
3. Multiply the number of moles of O₂ by the enthalpy change to find the heat produced.

By following these steps, you can find the heat for the decomposition of 432 kg of H₂O₂.