What can be inferred about the reaction from this information?
Why do the table temperatures fall from 1.0 to 6.0 minutes?
If temperature measurements had continued beyond 6.0 minutes, what lowest temperature would you expect to be reached?
Plot the table data onto the grid. Then draw a straight line of best fit and continue it until it crosses the $y$-axis.
On the grid, circle the anomalous point.
Use your graph to determine the mixture temperature at 2.5 minutes.
Use your graph to determine when the mixture temperature would be $30.0\,^{\circ}\text{C}$.
Use your graph to determine the mixture temperature at 0.0 minutes. This value is the highest temperature reached during the reaction.
The starting temperature of the aqueous iron(II) sulfate was $22.0\,^{\circ}\text{C}$. Calculate the greatest temperature increase after zinc is added.
Calculate the amount of substance, in moles, of iron(II) sulfate present in $25.0\,\text{cm}^3$ of $2.0\,\text{mol dm}^{-3}$ iron(II) sulfate.
The heat released in the reaction, in $\text{kJ mol}^{-1}$, is found from $\frac{25 \times 4.2 \times \text{maximum temperature rise}}{1000 \times \text{moles of iron(II) sulfate}}$. Apply this expression together with your answers to (d)(ii) and (e)(i) to determine the heat released in the reaction.