Nitrogen reacts with oxygen to make nitrogen monoxide.
N2+O2→2NO \mathrm{N_{2} + O_{2} \rightarrow 2NO} N2+O2→2NO| Bond | N≡N\mathrm{N{\equiv}N}N≡N | O=O\mathrm{O{=}O}O=O | N=O\mathrm{N{=}O}N=O |
|---|---|---|---|
| Bond energy (kJ/mol\mathrm{kJ/mol}kJ/mol) | 945 | 498 | 607 |
Statement 1: The energy taken in to break the bonds in the reactants is 1443 kJ/mol.
Statement 2: The energy released when the bonds in the products are made is 607 kJ/mol.
Statement 3: The reaction is endothermic.
Statement 4: The products have less energy than the reactants.
Which statements are correct?
1 and 3 only
1, 2 and 3 only
2 and 4 only
1, 3 and 4 only
51 exam-style questions on OCR GCSE Chemistry 3.2 Energetics, covering 3.2.1 Exothermic and endothermic reactions and reaction profiles and 3.2.2 Calculating energy change from bond energies. Each one has a worked solution and a mark scheme showing where the marks go.