Calculate the energy required to heat 702.0g of mercury from 2.6°C to 14.6°C. Assume the specific heat capacity of mercury under these conditions is ·0.139J·g−1K−1 . Be sure your answer has the correct number of significant digits.
Question
Calculate the energy required to heat 702.0g of mercury from 2.6°C to 14.6°C. Assume the specific heat capacity of mercury under these conditions is ·0.139J·g−1K−1 . Be sure your answer has the correct number of 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, and
- ΔT is the change in temperature.
Given:
- m = 702.0 g,
- c = 0.139 J/g·K, and
- ΔT = 14.6°C - 2.6°C = 12.0 K (Note: a change of 1°C is equivalent to a change of 1 K).
Substituting these values into the formula gives:
q = (702.0 g) * (0.139 J/g·K) * (12.0 K) = 1167.36 J
However, we need to consider the correct number of significant digits. The given values have four significant digits, so our final answer should also have four significant digits. Therefore, the energy required to heat 702.0 g of mercury from 2.6°C to 14.6°C is 1167 J.
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