Explain the results shown in Figure 3.
Do not refer to anomalous points.
Use data from Figure 3.

The graph shows that the reaction between zinc and copper sulfate is exothermic, as the temperature increases. - **Part 1 (Rising slope):** From 0.00 g to approximately 0.80 g of zinc, the temperature increases as more zinc is added. For instance, adding 0.20 g of zinc causes a temperature rise to 28°C, while adding 0.60 g causes a rise to 41°C. In this region, the zinc is the limiting reactant. This means there is an excess of copper sulfate, so adding more zinc allows more reaction to happen, releasing more thermal energy. - **Part 2 (Plateau):** After about 0.80 g of zinc, the temperature remains constant at approximately 47°C. At this point, the copper sulfate has become the limiting reactant. All of the copper sulfate has been used up, so even though more zinc is added, no further reaction can occur. Therefore, no more heat is produced, and the temperature does not increase further.