a 15.6g sample of ethanol absorbs 868J as it is heat. what is the temperature change of the ethanol? assume that the most specific heat is 2.44 J/g C. is this endothermic or exothermic?

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.