Gaseous hydrazine reacts with a gas X to form the gases nitrogen and HX by way of the following reaction:

NH (g)+2X (g)=N (g)+4HX(g)

The enthalpy change for Reaction 1 is −1180 kJ mol−1. Sketch or try and layout a fully labelled diagram showing how the internal energy changes for this reaction. On your diagram indicate the energy barrier for the reaction
Cheers,
jim

To sketch a fully labeled diagram showing the change in internal energy for this reaction, follow these steps:

1. Draw a horizontal line to represent the energy axis.
2. Label one side as "Reactants" and the other side as "Products" to indicate the two states of the reaction.
3. Indicate the initial energy level of the reactants and products on the respective sides of the diagram.
4. Draw a curve or a line connecting the energy levels for the reactants and products, representing the change in internal energy.
5. Label the curve or line as "Enthalpy Change = -1180 kJ mol^-1", indicating the value of the enthalpy change of the reaction.
6. Identify the energy barrier for the reaction by drawing a peak in the curve above the initial energy level of the reactants.
7. Label the energy barrier as the "Activation Energy", indicating that this is the minimum energy required for the reaction to proceed.
8. Optional: You can also label any additional energy changes along the reaction path, such as intermediate states or transition states.

Remember to label all the components clearly and provide a key if needed. This diagram will visually represent the change in internal energy during the reaction and show the energy barrier that must be overcome for the reaction to occur.