Question

Aluminum metal has a specific heat of 0.900 j/g·°c. Calculate the amount of heat required to raise the temperature of 10.5 moles of Al from 123.5 °C to 485 °C. (The unit of your answer should be kJ with 3 significant figures).

Answer 1

To calculate the heat required to raise the temperature of 10.5 moles of aluminum from 123.5 °C to 485 °C, convert moles to grams, calculate the change in temperature, and use the formula Q = m × C × ΔT. The heat required is approximately 94.01 kJ.

Step-by-step explanation:

To calculate the amount of heat required to raise the temperature of 10.5 moles of aluminum from 123.5 °C to 485 °C, we can use the formula:

Q = m × C × ΔT

where Q is the heat energy, m is the mass, C is the specific heat, and ΔT is the change in temperature.

First, we need to convert moles to grams using the molar mass of aluminum (26.98 g/mol). Therefore, the mass of aluminum is 10.5 moles × 26.98 g/mol = 283.29 g.

Next, we calculate the change in temperature: ΔT = 485 °C - 123.5 °C = 361.5 °C.

Finally, we can calculate the heat energy using the formula Q = 283.29 g × 0.900 J/g·°C × 361.5 °C = 94,010.43 J = 94.01 kJ (rounded to 3 significant figures).