Multiple Choice
If 14.5 kJ of heat is added to 485 g of liquid water, how much will the temperature of the water increase? (Assume the specific heat capacity of water is 4.18 J/g·°C.)
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8. Thermochemistry
Heat Capacity
Multiple Choice
50.00 g of heated metal ore is placed into an insulated beaker containing 822.5 g of water. Once the metal heats up the final temperature of the water is 32.08 ºC. If the metal gains 14.55 kJ of energy, what is the initial temperature of the water?
A
23.86 °C
B
32.86 °C
C
63.08 °C
D
36.31 °C
Verified step by step guidance1
Identify the known values: mass of water (mwater) = 822.5 g, final temperature of water (Tfinal) = 32.08 °C, energy gained by metal (qmetal) = 14.55 kJ.
Convert the energy gained by the metal from kilojoules to joules: 14.55 kJ = 14550 J.
Use the formula for heat transfer: q = m × c × ΔT, where q is the heat absorbed or released, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
Rearrange the formula to solve for the initial temperature of the water (Tinitial): Tinitial = Tfinal - (q / (mwater × cwater)).
Substitute the known values into the equation: Tinitial = 32.08 °C - (14550 J / (822.5 g × 4.18 J/g°C)), where 4.18 J/g°C is the specific heat capacity of water.
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