How much heat energy is released when 150.0 g of water is cooled from 45.0 °C to 12.5 °C? The specific heat capacity of water is 4.18 J/g°C.Question 7Select one:a.-28200 Jb.-20400 Jc.-11700 Jd.-36100 J
Question
How much heat energy is released when 150.0 g of water is cooled from 45.0 °C to 12.5 °C? The specific heat capacity of water is 4.18 J/g°C.Question 7Select one:a.-28200 Jb.-20400 Jc.-11700 Jd.-36100 J
Solution
To solve this problem, we need to use the formula for heat transfer:
q = mcΔT
where:
- q is the heat energy,
- m is the mass of the substance,
- c is the specific heat capacity, and
- ΔT is the change in temperature.
Given:
- m = 150.0 g,
- c = 4.18 J/g°C, and
- ΔT = 45.0 °C - 12.5 °C = 32.5 °C.
Substituting these values into the formula gives:
q = (150.0 g)(4.18 J/g°C)(32.5 °C) = 20362.5 J
Since heat is being released as the water cools, we consider q to be negative. So, q = -20362.5 J.
Rounding to the nearest hundred gives us -20400 J. So, the answer is (b) -20400 J.
Similar Questions
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