4. how many j of energy are needed to raise the temperature of 165 g of water from 10.55°c to 47.32°c?

Q = 25360.269 j

Explanation:

Given data:

Mass = 165 g

Initial temperature = 10.55 °C

Final temperature = 47.32°C

Energy absorbed = ?

Solution:

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT  = T2 - T1

ΔT  = 47.32°C - 10.55 °C

ΔT  = 36.77 °C

Q = m.c. ΔT

Q = 165 g . 4.18 j/g.°C . 36.77 °C

Q = 25360.269 j

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.