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Answer :
Final answer:
The energy required to heat 825.0 g of water from 26.0°C to 38.4°C is 41,091 J.
Explanation:
To calculate the energy required to heat the water, we can use the formula:
Q = mcΔT
Where:
- Q is the heat energy
- m is the mass of the substance
- c is the specific heat capacity
- ΔT is the change in temperature
Given:
- Mass of water (m) = 825.0 g
- Specific heat capacity of water (c) = 4.18 J/g/K
- Initial temperature (T1) = 26.0°C
- Final temperature (T2) = 38.4°C
First, we need to calculate the change in temperature:
ΔT = T2 - T1 = 38.4°C - 26.0°C = 12.4°C
Now, we can substitute the values into the formula:
Q = (825.0 g) * (4.18 J/g/K) * (12.4°C)
Calculating the value:
Q = 41,091 J
Therefore, the energy required to heat 825.0 g of water from 26.0°C to 38.4°C is 41,091 J.
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