Identify the oxidising agent in this reaction. Justify your answer with oxidation numbers.
Suggest one observation you would make, ignoring any temperature change, when bromine reacts with methanoic acid.
Use the graph to work out the average rate of reaction at $20\,^{\circ}\text{C}$ during the first $600\,\text{s}$. State the units for this rate of reaction.
Sketch a graph on the same axes to show the expected outcome when the experiment is repeated at $40\,^{\circ}\text{C}$.
The rate of reaction increases when the number of successful collisions between reactant particles rises. Explain why increasing the temperature produces this effect.
Complete the ‘dot-and-cross’ diagram, showing outer electrons only, to illustrate the bonding in methanoic acid, $\text{HCO}_2\text{H}$.