1. **State the problem:** Calculate the energy required to heat 480.0 g of copper from 14.84 °C to 25.49 °C given the specific heat of copper is 0.3850 J/(g·°C). 2. **Formula used:** The heat equation is $$q = m \times \Delta T \times SH$$ where: - $q$ is the heat energy (Joules), - $m$ is the mass (grams), - $\Delta T$ is the change in temperature (°C), - $SH$ is the specific heat (J/(g·°C)). 3. **Calculate the temperature change:** $$\Delta T = T_{final} - T_{initial} = 25.49 - 14.84 = 10.65\,°C$$ 4. **Substitute values into the heat equation:** $$q = 480.0 \times 10.65 \times 0.3850$$ 5. **Calculate intermediate multiplication:** $$q = 480.0 \times \cancel{10.65} \times 0.3850 = 480.0 \times 4.10025$$ 6. **Final calculation:** $$q = 1968.12\,J$$ 7. **Express answer to four significant figures:** $$q = 1968\,J$$ **Answer:** It takes 1968 J of energy to heat the copper tubing. --- **Note:** Part B is a conceptual explanation about exothermic and endothermic reactions and does not require calculation here.