How much energy (in JJ) is lost when a sample of iron with a mass of 29.2 gg cools from 79.0 ∘C∘C to 27.0 ∘C∘C?

- 0.674 kJ.

Explanation:

The equation used to solve this problem is:

Q = mCΔT

where,

Q = amount of heat

m = mass of the substance

C = specific heat capacity

ΔT = change in temperature

= Temp.f - Temp.i

Given:

m = 29.2 g

Temp.i = 79°C

Temp.f = 27°C

Cp(iron) = 0.444 J/g.K

Q = mCΔT

ΔT = 27.0°C - 79.0°C

= -52°C

= 29.2 * 0.444 * -52

Q = - 674.17 J

= 0.674 kJ.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.

it’s previous models   because when i picked that son of a gun’s answer it was wrong look for previous models because they might make it a different letter