Multiple Choice
Which amount of energy is required to raise the temperature of one gram of water by one degree Celsius?
8. Thermochemistry
Heat Capacity
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A sample of copper absorbs 3.53 kJ of heat, which increases the temperature by 25 ºC, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J / g ºC.
A
0.73 kg
B
0.35 kg
C
0.37 kg
D
0.53 kg
Verified step by step guidance1
Identify the formula to use: The heat absorbed or released by a substance can be calculated using the formula \( q = m \cdot c \cdot \Delta T \), where \( q \) is the heat absorbed, \( m \) is the mass, \( c \) is the specific heat capacity, and \( \Delta T \) is the change in temperature.
Convert the heat absorbed from kilojoules to joules: Since the specific heat capacity is given in J/g·°C, convert 3.53 kJ to joules by multiplying by 1000. Thus, \( q = 3.53 \times 1000 \) J.
Rearrange the formula to solve for mass \( m \): \( m = \frac{q}{c \cdot \Delta T} \).
Substitute the known values into the rearranged formula: \( q = 3530 \) J, \( c = 0.385 \) J/g·°C, and \( \Delta T = 25 \) °C.
Calculate the mass in grams and then convert it to kilograms by dividing by 1000. This will give you the mass of the copper sample in kg.
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