Answer :
Final answer:
The energy change when the temperature of 0.550 kg of water decreased from 103 °C to 33.0 °C is -13.3 kJ.
Explanation:
To determine the energy change when the temperature of 0.550 kg of water decreased from 103 °C to 33.0 °C, we can use the equation:
Q = mcΔT
Where Q is the energy change, m is the mass of water, c is the specific heat capacity of water, and ΔT is the change in temperature.
Given:
- Mass of water (m) = 0.550 kg
- Initial temperature (T1) = 103 °C
- Final temperature (T2) = 33.0 °C
- Specific heat capacity of water (c) = 4.184 J/g °C
First, convert the mass of water to grams:
0.550 kg × 1000 g/kg = 550 g
Next, calculate the change in temperature:
ΔT = T2 - T1 = 33.0 °C - 103 °C = -70.0 °C
Finally, plug in the values into the equation:
Q = (550 g)(4.184 J/g °C)(-70.0 °C) = -1.33 × 10^4 J
Since the question asks for the energy change in kJ, we can convert the answer:
-1.33 × 10^4 J = -13.3 kJ
Therefore, the energy change when the temperature of 0.550 kg of water decreased from 103 °C to 33.0 °C is -13.3 kJ.
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