CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔH=−882.kJ

asked by @students3940 • 10 months ago • Chemistry • 5 pts

A chemist measures the energy change ΔH during the following reaction: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔH=−882.kJ

Use the information to answer the following questions. 1) Is it endothermic or exothermic? 2) 41.1g of CH4 react. Will any heat be released or absorbed? 3) 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 in kJ

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1 answer

1.Negative DH indicates an Exothermic reaction, where energy is released. 2. Heat will be released 3. You can say that -882.kJ will be released per 1 mole of CH4, the molar mass of CH4 is 16 g/mol, if you have 41.1g of CH4, you will have 2.6 mols of CH4.

DH is -882.kJ/ mol CH4, times this by your moles of CH4 to get the amount of energy produced, -2,293.2 or -2,300 kJ (Sig figs)

answered by @bohdanh1 • 10 months ago
  • Hey @bohdanh1! Thank you for answering Reyn commented 10 months ago