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.