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Calculate the amount of heat (in kJ) required to heat 244 g of Al(s) from 22.2 °C to 39.3 °C. Enter the value using the correct number of significant figures in decimal form.

Answer :

Final answer:

The heat energy required to raise the temperature of 244 g of aluminum from 22.2 °C to 39.3 °C is 3.76 kJ, considering aluminum's specific heat capacity is 900 J/kg·°C.

Explanation:

To calculate the amount of heat (in kJ) required to heat 244 g of Al(s) from 22.2 °C to 39.3 °C, we will use the formula: Q = m·c·∆T, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ∆T is the change in temperature. The specific heat capacity of aluminum is 900 J/kg·°C.

First, convert the mass from grams to kilograms: 244 g = 0.244 kg. Then, calculate the change in temperature: 39.3 °C - 22.2 °C = 17.1 °C. Now, substitute the values into the formula: Q = (0.244 kg) · (900 J/kg·°C) · (17.1 °C). Upon calculation: Q = 3760.356 kJ. However, we need to convert this to kJ and use the correct number of significant figures: 3.76 kJ.

This is the amount of heat energy required to heat 244 g of aluminum from 22.2 °C to 39.3 °C. Note that in determining the significant figures, we look at the initial temperature values given which have three significant figures. Therefore, our final answer should be reported with three significant figures as well.

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