This question is about the reaction between methane (CH4\text{CH}_4CH4) and oxygen (O2\text{O}_2O2).
The equation for the reaction is: CH4(g)+2O2(g)→CO2(g)+2H2O(g)\text{CH}_4(\text{g}) + 2\text{O}_2(\text{g}) \rightarrow \text{CO}_2(\text{g}) + 2\text{H}_2\text{O}(\text{g})CH4(g)+2O2(g)→CO2(g)+2H2O(g)
What does H2O(g)\text{H}_2\text{O}(\text{g})H2O(g) represent?
Calculate the volume of oxygen required to react with 45 cm345\text{ cm}^345 cm3 of methane.
The reaction is exothermic.
Complete the reaction profile shown below:
You should:
- complete the profile line
- label the activation energy (EaE_aEa)
- label the overall energy change (ΔH\Delta HΔH).
The displayed formula equation for the reaction of methane with oxygen is: H−∣HH∣-H + 2 O=O → O=C=O + 2 H−O−H\text{H}-\underset{\overset{|}{\text{H}}}{\overset{\text{H}}{|}}\text{-H} \ + \ 2\ \text{O}=\text{O} \ \rightarrow \ \text{O}=\text{C}=\text{O} \ + \ 2\ \text{H}-\text{O}-\text{H}H−H∣∣H-H + 2 O=O → O=C=O + 2 H−O−H
The table below shows some of the bond energies:
| Bond | C−H\text{C}-\text{H}C−H | O=O\text{O}=\text{O}O=O | C=O\text{C}=\text{O}C=O | O−H\text{O}-\text{H}O−H |
|---|---|---|---|---|
| Bond Energy (kJ/mol) | XXX | 495495495 | 799799799 | 463463463 |
In the reaction, the energy released forming new bonds is 812 kJ/mol812\text{ kJ/mol}812 kJ/mol greater than the energy needed to break existing bonds.
Calculate the bond energy XXX for the C−H\text{C}-\text{H}C−H bond.