What is the final temperature when 625 grams of water at 75.0 C loses 7.96 x 10 to the fourth power J ? The specific heat of water is 4.18 J/gC

The final temperature of the water was 44.5 °C

Let the final temperature be F. Therefore:

Heat lost = mass * specific heat of water * change in temperature

-7.96 * 10⁴ = 625 g * 4.18 J/gC * (F - 75)

F - 75 = -30.5

F - 75 + 75 = -30.5 + 75

F = 44.5 °C

Hence the final temperature of the water was 44.5 °C

Find out more at: link

The final temperature : 44.5 °C

Heat can be formulated :

Q = m . c .Δt

Q = heat, J

m = mass, g

c = specific heat, J/gC

Δt= temperature

m= 625 g

Q=7.96 x 10⁴ J

c = 4.18 j/gC

t₁=75 C

a non redox reaction occurs when there is not a transfer of electrons. for redox reactions, which are reduction-oxidation reactions, a change in the oxidation number occurs. elements that are reduced gain electrons, and elements that are oxidized lose electrons.

explanation:

level 4 to level 2 : ))