How much heat is required to raise the temperature of
12.0
g
of water from
−
35

°C
to
175

°C?

heat:
kcal

Q = 1.68 Kcal

Explanation:

∴ m H2O = 12.0 g

∴ T1 = 35°C ≅ 308 K

∴ T2 = 175°C ≅ 448 K

∴ ΔT = T2 - T1 = 175 - 35 = 140 °C

∴ Cp H2O = 1 cal /g.°C

⇒ Q = (12.0 g)(1 cal/g°C)(140 °C)

⇒ Q = (1680 cal)*(Kcal/1000 cal)

⇒ Q = 1.68 Kcal

it means there are 3 atoms of oxygen

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.