The Temperature Change of Ethanol in a Heating Process
Calculation of Temperature Change in Ethanol Heating Process
A 15.6g sample of ethanol absorbs 868J as it is heat. What is the temperature change of the ethanol? Assume that the specific heat is 2.44 J/g°C.
Answer:
Change in temperature, ΔT = 22.8°C
Reaction is endothermic.
Explanation:
The amount heat is given by the formula;
q = m×c×ΔT
Where, q is the amount of heat, m is the mass of a substance, c is the specific heat capacity, ΔT is the temperature change.
In this case, making ΔT the subject of the formula, we get;
ΔT = q/m×c
But; q = 868 Joules, m = 15.6 g, c = 2.44 J/g°C
Therefore;
ΔT = 868 J / (2.44 J/g°C × 15.6 g)
= 22.8 °C
Therefore, the temperature change for ethanol is 22.8 °C. This means there is an increase in temperature, and therefore the reaction is endothermic.
Question:
Is the heating process of ethanol described in the data endothermic or exothermic? And what is the calculated temperature change?
Answer:
The heating process of ethanol is endothermic, and the calculated temperature change is 22.8°C.