How much energy is required to change 150.0 g of water from 10.0°C to 45.0°C? (Cwater = 4.18 J/g • °C)A 125.4 JB 627.0 JC 21900 JD 28200 J
Question
How much energy is required to change 150.0 g of water from 10.0°C to 45.0°C?
(C<sub>water</sub> = 4.18 J/g • °C)
A. 125.4 J
B. 627.0 J
C. 21900 J
D. 28200 J
Solution
To solve this problem, we need to use the formula for calculating heat energy, which is:
q = mcΔT
where:
- q is the heat energy
- m is the mass of the substance (in this case, water)
- c is the specific heat capacity of the substance (for water, it's given as 4.18 J/g°C)
- ΔT is the change in temperature
Given: m = 150.0 g c = 4.18 J/g°C ΔT = 45.0°C - 10.0°C = 35.0°C
Substituting these values into the formula, we get:
q = (150.0 g) * (4.18 J/g°C) * (35.0°C) = 21945 J
So, the amount of energy required to change 150.0 g of water from 10.0°C to 45.0°C is approximately 21945 J. The closest answer to this is D) 28200 J.
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