This question is about the reaction between nitrogen gas (N2\text{N}_2N2) and hydrogen gas (H2\text{H}_2H2) to form ammonia (NH3\text{NH}_3NH3).
The equation for the reaction is: N2(g)+3H2(g)→2NH3(g)\text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightarrow 2\text{NH}_3(\text{g})N2(g)+3H2(g)→2NH3(g)
What does NH3(g)\text{NH}_3(\text{g})NH3(g) represent?
Calculate the volume of hydrogen gas required to react completely with 45 cm345\text{ cm}^345 cm3 of nitrogen gas.
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 nitrogen with hydrogen is: N≡N + 3 H−H → 2 H−N∣H−H\text{N}\equiv\text{N} \ + \ 3\ \text{H}-\text{H} \ \rightarrow \ 2 \ \text{H}-\underset{\text{H}}{\underset{|}{\text{N}}}-\text{H}N≡N + 3 H−H → 2 H−H∣N−H
The table below shows some of the bond energies:
| Bond | N≡N\text{N}\equiv\text{N}N≡N | H−H\text{H}-\text{H}H−H | N−H\text{N}-\text{H}N−H |
|---|---|---|---|
| Bond Energy (kJ/mol) | 945945945 | 436436436 | XXX |
In the reaction, the energy released forming new bonds is 93 kJ/mol93\text{ kJ/mol}93 kJ/mol greater than the energy needed to break existing bonds.
Calculate the bond energy XXX for the N−H\text{N}-\text{H}N−H bond.