# What is the final temperature of water

I got achem test tomororw and 2 questions didn't have asnwers for them so i want to make sure of them.

1) If 335 g of water at 24.5 degrees Celcius absorbed 2.66 kJ of energy, what is the final temperature of water

*2.66 = 335 * 4.184 * t + 24.5 (or 24.5 - t)? dont know

and

2)7.28 kJ of heat is released when 40.9 g of Br2 (bormine) vapour at 332 K condense to a liquid. What is the molar heat of vaporization of Br2.

i just want to make sure i got the right asnwers, cause these 2 don't have asnwers in our test revision sheet. thanks

mrjeffy321
For these two problems you need to remember two of the heat energy formulas,
Q = m*C*T
And
Q = m*L
Where Q is the heat energy, m is the mass, C is the specific heat, T is the change in temperature, and L is the Latent heat [of vaporization].

For your first problem, you need to remember to keep the units on your energy straight, or the prefixes atleast.
2.66 kJ of energy are absorbed, but the specific heat your using for water is 4.184 J/g*degree C
So you need to convert one or the other to get the right answer.
So then just solve for the change in temperature.
2660 J = 335 g * 4.184 J/gC * T

You know the energy given off and the mass of the bromine giving it off, so just solve for the latent heat.
7280 J = 40.9 g * L

god bless u mr. jeffey
for the 2nd prob tho, is the 332K insignifcant
dont i have to find out the heat it takes to get to its vap. piont first.

mrjeffy321