how do I figure out the final temperature? The AH for the solution process when
ID: 893159 • Letter: H
Question
how do I figure out the final temperature? The AH for the solution process when solid sodium hydroxide dissolves in water is 44.4 kj/mol. What amount of NaOH dissolves in 250.0g of water in a coffee-cup calorimeter that causes a temperature increase from 24.0 degree C to 39.0 degree C? Assume the solution has the same specific heat as liquid water (4.18 J/g degree C). A 5.00g sample of copper has an initial temperature of 95 degree C The initial temperature for a 25.0g sample of water is 22.5 C What is the final temperature of this mixture? Specific heat of copper is 0.385 |/g ^aC The combustion of titanium with oxygen produces titanium (IV) oxide: Tl (s) o2 (g) -> TIo^2 (s) f 1.750g of titanium is combusted In a bornb calorimeter, the temperature of the calorimeter increases from 25.0*C to 93.6 degree C. If in a separate experiment, the heat capacity of the calorimeter is determined to be 9.84 k|/ degree C calculate the heat of reaction for the combustion per mole of Ti (kl/mol).Explanation / Answer
10 .
specific heat of water s = 4.18 J/(gC)
mass of water = 250 grams
DT = 39-24 = 15
q absorbed by water = m*s*DT
= 250*4.18*15 = 15.675 kj
from the data 1 mole = 44.4 kj
so that ? mole = 15.675 kj
= 15.675/44.44 = 0.3528 mole
mass of NaOH = 0.3528*40 = 14.112 grams
11.
qmetal lost = q water absorbed
m*s*DT = m*s*DT
5*0.385*(95-Tf) = 25*4.18*(Tf-22.5)
Tf= final temperature of mixer = 23.811 c
12.
heat capacity of calorimeter = 9.84 kj/C
heat absorbed = 9.84*(93.6-25) = 675.024 kj
No of moles of Ti = 1.75/47.867 = 0.03656 mole
heat of reaction = 675.024/0.03656 = 18463.457 kj/mol
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