A chemist measures the energy change ΔH during the following reaction:2H2O(l)→2H2(g)+O2(g) =ΔH572.kJUse the information to answer the following questions.This reaction is... endothermic.exothermic.Suppose 56.7g of H2O react.Will any heat be released or absorbed?Yes, absorbed.Yes, released.No.If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. kJBe sure your answer has the correct number of significant digits.
Question
A chemist measures the energy change ΔH during the following reaction:2H2O(l)→2H2(g)+O2(g) =ΔH572.kJUse the information to answer the following questions.This reaction is... endothermic.exothermic.Suppose 56.7g of H2O react.Will any heat be released or absorbed?Yes, absorbed.Yes, released.No.If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. kJBe sure your answer has the correct number of significant digits.
Solution
The reaction is endothermic because the energy change ΔH is positive, which means energy is absorbed from the surroundings.
Given that the molar mass of H2O is approximately 18.015 g/mol, 56.7 g of H2O is equivalent to 56.7 g / 18.015 g/mol = 3.15 mol.
The reaction equation shows that 2 mol of H2O absorb 572 kJ of heat. Therefore, 1 mol of H2O would absorb 572 kJ / 2 = 286 kJ of heat.
So, 3.15 mol of H2O would absorb 3.15 mol * 286 kJ/mol = 901.7 kJ of heat.
Therefore, the heat absorbed is 901.7 kJ.
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