QuestionMay 7, 2025

Calculate the energy required to heat 0.40 kg of ethanol from -3.4^circ C to 11.6^circ C Assume the specific heat capacity of ethanol under these conditions is 2.44Jcdot g^-1cdot K^-1 . Be sure your answer has the correct number of significant digits. square

Calculate the energy required to heat 0.40 kg of ethanol from -3.4^circ C to 11.6^circ C Assume the specific heat capacity of ethanol under these conditions is 2.44Jcdot g^-1cdot K^-1 . Be sure your answer has the correct number of significant digits. square
Calculate the energy required to heat 0.40 kg of ethanol from -3.4^circ C to 11.6^circ C Assume the specific heat capacity of ethanol under these conditions is 2.44Jcdot g^-1cdot K^-1 . Be sure your answer has the correct number of significant digits. square

Solution
4.6(182 votes)

Answer

1.46 \times 10^4 \, \text{J} Explanation 1. Convert mass to grams 0.40 \, \text{kg} = 400 \, \text{g} 2. Calculate temperature change \Delta T = 11.6 - (-3.4) = 15.0 \, \text{K} 3. Apply heat energy formula Use Q = m \cdot c \cdot \Delta T, where m = 400 \, \text{g}, c = 2.44 \, \text{J} \cdot \text{g}^{-1} \cdot \text{K}^{-1}, and \Delta T = 15.0 \, \text{K}. Q = 400 \cdot 2.44 \cdot 15.0 = 14,640 \, \text{J} 4. Adjust significant digits The given values have 3 significant digits, so the answer must also have 3 significant digits.

Explanation

1. Convert mass to grams<br /> $0.40 \, \text{kg} = 400 \, \text{g}$<br /><br />2. Calculate temperature change<br /> $\Delta T = 11.6 - (-3.4) = 15.0 \, \text{K}$<br /><br />3. Apply heat energy formula<br /> Use $Q = m \cdot c \cdot \Delta T$, where $m = 400 \, \text{g}$, $c = 2.44 \, \text{J} \cdot \text{g}^{-1} \cdot \text{K}^{-1}$, and $\Delta T = 15.0 \, \text{K}$.<br /> $Q = 400 \cdot 2.44 \cdot 15.0 = 14,640 \, \text{J}$<br /><br />4. Adjust significant digits<br /> The given values have 3 significant digits, so the answer must also have 3 significant digits.
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