Question

When 0.500 g CaO(s) is added to 140. g H2O at 23.1 °C in a coffee...

When 0.500 g CaO(s) is added to 140. g H2O at 23.1 °C in a coffee cup calorimeter, this reaction occurs.

CaO(s)+H2O(l)-->Ca(OH)2 (aq) and enthalpy = -81.9 kj/mol

Calculate the final temperature of the solution. The specific heat capacity of water is 4.184

Homework Answers

Answer #1

Hrxn = -81.9 kJ/mol

mol of CaO = mass/MW = 0.5/56.0774 = 0.0089162479 mol of CaO

mol of H2O = mass/MW = 140/18 = 7.777 mol of H2O

since CaO is limiting

then

0.0089162479 mol should be used

Q = nHRxn = 0.0089162479 *-81.9 = -0.73024070301kJ = -730.240 kJ

note that this is EXOthermic, meaning this will increase the temperature of the system (i.e.calorimeter)

then

Q = m*Cp*dT

Q = 730.240 J

mT = 0.5+140 = 140.5 g

Cp = 4.184J/gC (approx of water)

dT = Tf- 23.1

Q = m*Cp*dT = (140.5)(4.184)(Tf-23.1) = 730.240

(140.5)(4.184)(Tf-23.1) = 730.240

Tf = 730.240 /(140.5*4.184) + 23.1 = 24.3422

Tf = 24.3422 °C

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
When 23.8 mL of 0.500 M H2SO4 is added to 23.8 mL of 1.00 M KOH...
When 23.8 mL of 0.500 M H2SO4 is added to 23.8 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g·°C.) ?: kJ/mol H2O
When 7.56 g of NaCl is added to a coffee cup calorimeter, the water temperature changes...
When 7.56 g of NaCl is added to a coffee cup calorimeter, the water temperature changes by 4.1 ºC. If the heat of solution (the enthalpy change upon dissolving in water) is 3.8 kJ/mol, what mass of solution must be in the cup? Assume the specific heat capacity of the solution is the same as the specific heat capacity of water.
When 0.109 g of Zn(s) combines with enough HCl to make 55.7 mL of HCl(aq) in...
When 0.109 g of Zn(s) combines with enough HCl to make 55.7 mL of HCl(aq) in a coffee cup calorimeter, all of the zinc reacts, which increases the temperature of the HCl solution from 23.2 °C to 24.8 °C: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) Calculate the enthalpy change of the reaction ΔHrxn in J/mol. Insert your answer in kJ, but do not write kJ after the number. (Assume the density of the solution is 1.00 g/mL and the...
Enter your answer in the provided box. When 22.9 mL of 0.500 M H2SO4 is added...
Enter your answer in the provided box. When 22.9 mL of 0.500 M H2SO4 is added to 22.9 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17 °C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water =...
In the following experiment, a coffee-cup calorimeter containing 100. mL of H2O is used. The initial...
In the following experiment, a coffee-cup calorimeter containing 100. mL of H2O is used. The initial temperature of the calorimeter is 23.0 ∘C. If 2.00 g of CaCl2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution, ΔHsoln, of CaCl2 is −82.8 kJ/mol. The specific heat of water is CS=4.184 J/(g−K
When 0.113 g of Zn(s) combines with enough HCl to make 53.6 mL of HCl(aq) in...
When 0.113 g of Zn(s) combines with enough HCl to make 53.6 mL of HCl(aq) in a coffee cup calorimeter, all of the zinc reacts, which increases the temperature of the HCl solution from 23.3 °C to 24.7 °C: Zn(s) + 2HCl(aq) → ZnCl2​(aq) + H2​(g) Calculate the enthalpy change of the reaction ΔHrxn​ in J/mol. Insert your answer in kJ, but do not write kJ after the number. (Assume the density of the solution is 1.00 g/mL and the...
When 0.100 g Zn(s) combines with enough HCl to make a total of 55.0 mL solution...
When 0.100 g Zn(s) combines with enough HCl to make a total of 55.0 mL solution in a coffee cup calorimeter, all of the zinc reacts, which increases the temperature of the HCl solution from 23.0∘C to 24.5 ∘C: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) Calculate the enthalpy change of the reaction ΔHrxn. (Assume the density of the solution is 1.00 g/mL and the specific heat capacity of solution is 4.184 J/g∘C.) in J/mol. (Enter answer in numerical form...
When 26.5 mL of 0.500 M H2SO4 is added to 26.5 mL of 1.00 M KOH...
When 26.5 mL of 0.500 M H2SO4 is added to 26.5 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50° C, the temperature rises to 30.17° C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g°C). Answer in kJ/molH2O
50.0 mL of 0.100 M KOH, at 20.00o C, is added to 50.00 mL of 0.110...
50.0 mL of 0.100 M KOH, at 20.00o C, is added to 50.00 mL of 0.110 M HCl, at 20.00o C, in a coffee cup calorimeter. The enthalpy of neutralization is 56.0 kJ/mol. The specific heat capacity of the total solution is 4.184 Jg-1 oC-1, and the density of the total solution is 1.00 g/mL, what is Tf for the reaction?
When 4.50 g of Ba(s) is added to 100.00 g of water in a container open...
When 4.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 54.35°C. If the specific heat of the solution is 4.18 J/(g • °C), calculate ΔH for the reaction, as written. Ba(s) + 2 H2O(l) → Ba(OH)2(aq) + H2(g) ΔH = ? When 4.50 g of Ba(s) is added to 100.00 g of water in a...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT