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Answer :
Final answer:
The energy change when 0.250 kg of water cools from 115 °C to 25.0 °C is -94,695 J, which means the water loses this amount of energy.
Explanation:
The energy change when the temperature of 0.250 kg of water decreases from 115 °C to 25.0 °C, we use the specific heat capacity of water and the formula:
Q = mcΔT
where:
- Q is the energy in joules,
- m is the mass of the water in kilograms,
- c is the specific heat capacity of water (4.186 J/g°C), and
- ΔT is the change in temperature in Celsius.
First, we convert the specific heat capacity to J/kg°C because our mass is in kilograms:
4.186 J/g°C × 1000 g/kg = 4186 J/kg°C
Now we can calculate the change in temperature (ΔT):
ΔT = 25.0 °C - 115 °C = -90 °C
And the energy change (Q):
Q = 0.250 kg × 4186 J/kg°C × (-90 °C)
Q = -94,695 J
The negative sign indicates that energy is being lost from the water as it cools.
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