If 400 J of energy is added to 10 grams of water (specific heat capacity = 4.18 J/g·°C), what is the resulting temperature change?

• A. 9.6 °C
• B. 0.96 °C
• C. 4.18 °C
• D. 1.0 °C

Answer: (A)

Verified step by step guidance

1. Identify the known values from the problem: the energy added \(q = 400\ \text{J}\), the mass of water \(m = 10\ \text{g}\), and the specific heat capacity of water \(c = 4.18\ \text{J/g} \cdot ^\circ\text{C}\).
2. Recall the formula that relates heat energy to temperature change: \(q = m \times c \times \Delta T\), where \(\Delta T\) is the temperature change.
3. Rearrange the formula to solve for the temperature change \(\Delta T\): \(\Delta T = \frac{q}{m \times c}\).
4. Substitute the known values into the rearranged formula: \(\Delta T = \frac{400}{10 \times 4.18}\).
5. Calculate the value of \(\Delta T\) to find the temperature change in degrees Celsius.