Final answer:
To calculate the heat absorbed by 0.463 g of ethanol for a temperature increase from 51.6 °C to 82.4 °C, we use the specific heat capacity of ethanol (2.42 J/g°C) and the formula q = m × c × ΔT, obtaining approximately 34.43 joules of heat absorbed.
Step-by-step explanation:
The student has asked to calculate the amount of heat required to change the temperature of a given mass of ethanol using its specific heat capacity. To find the heat absorbed, we use the formula q = m × c × ΔT, where:
- q is the heat absorbed (in joules, J),
- m is the mass of the substance (in grams, g),
- c is the specific heat capacity (in J/g°C),
- ΔT is the change in temperature (in °C).
For 0.463 g of ethanol (m) with a specific heat capacity of 2.42 J/g°C (c), and a temperature change (ΔT) from 51.6°C to 82.4°C, the calculation is as follows:
q = (0.463 g) × (2.42 J/g°C) × (82.4°C - 51.6°C)
q = (0.463 g) × (2.42 J/g°C) × (30.8°C) = 34.42536 J
The heat absorbed is approximately 34.43 joules.