Calculate the energy required to heat 101.0mg of ethanol from 17.8°C to 24.0°C. Assume the specific heat capacity of ethanol under these conditions is ·2.44J·g−1K−1 . Round your answer to 2 significant digits.
Question
Calculate the energy required to heat 101.0mg of ethanol from 17.8°C to 24.0°C. Assume the specific heat capacity of ethanol under these conditions is ·2.44J·g−1K−1 . Round your answer to 2 significant digits.
Solution
To calculate the energy required to heat a substance, you 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 of the substance
- ΔT is the change in temperature
First, convert the mass from milligrams to grams:
101.0 mg = 0.101 g
Next, calculate the change in temperature:
ΔT = T_final - T_initial = 24.0°C - 17.8°C = 6.2°C
Now, substitute the values into the formula:
q = (0.101 g) * (2.44 J/g·K) * (6.2 K) = 1.50 J
So, the energy required to heat 101.0 mg of ethanol from 17.8°C to 24.0°C is approximately 1.50 J.
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