Calculate the energy required to heat 142.0g of iron from −4.8°C to 19.2°C. Assume the specific heat capacity of iron under these conditions is ·0.449J·g−1K−1 . Round your answer to 3 significant digits.
Question
Calculate the energy required to heat 142.0g of iron from −4.8°C to 19.2°C. Assume the specific heat capacity of iron under these conditions is ·0.449J·g−1K−1 . Round your answer to 3 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 = 142.0 g,
- c = 0.449 J/g·K, and
- ΔT = 19.2°C - (-4.8°C) = 24.0 K (note that a change of 1°C is equivalent to a change of 1 K).
Substituting these values into the formula gives:
q = (142.0 g) * (0.449 J/g·K) * (24.0 K) = 1525.632 J
Rounding to three significant digits gives q = 1520 J. So, the energy required to heat 142.0 g of iron from -4.8°C to 19.2°C is 1520 J.
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