Multiple Choice
A 100 g sample of water at 25 °C is cooled to 0 °C. How much energy must be transferred out of the system as heat (q) to lower its temperature to 0 °C? (Specific heat capacity of water = 4.18 J/g·°C)
8. Thermochemistry
Heat Capacity
Multiple Choice
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
Verified step by step guidance1
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 \(c = 4.18\ \text{J/g} \cdot ^\circ\text{C}\).
Recall the formula that relates heat energy to temperature change: \(q = m \times c \times \Delta T\), where \(\Delta T\) is the temperature change.
Rearrange the formula to solve for the temperature change \(\Delta T\): \(\Delta T = \frac{q}{m \times c}\).
Substitute the known values into the rearranged formula: \(\Delta T = \frac{400}{10 \times 4.18}\).
Calculate the value of \(\Delta T\) to find the temperature change in degrees Celsius.
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