Question

When a 2.00 g sample of KCl is dissolved in water in a calorimeter that has...

When a 2.00 g sample of KCl is dissolved in water in a calorimeter that has a total heat capacity of 1.538 kJ/K, the temperature decreases by 0.300 K. Calculate the molar heat of solution of KCl.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Heat absorbed by water = heat capacity of calorimeter*t

                                 = 1.538*0.3 = 0.4614 kj

no of moles of KCl = weight of KCl/Gram molar mass

                            = 2/74.6 = 0.0268 moles

molar heat of KCl solution = 0.4614/0.0268 = 17.21kj/mole

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
When a 3.00-g sample of KSCN is dissolved in water in a calorimeter that has a...
When a 3.00-g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 1.966 kJ·K–1, the temperature decreases by 0.380 K. Calculate the molar heat of solution of KSCN.​
A 0.505 g sample of KCl is added to 61.0 g of water in a calorimeter....
A 0.505 g sample of KCl is added to 61.0 g of water in a calorimeter. If the temperature decreases by 1.06°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C?
A 2.00 g sample of KCl is added to 35.0 g H2O in a styrofoam cup...
A 2.00 g sample of KCl is added to 35.0 g H2O in a styrofoam cup and stirred until dissolved. The temperature of the solution drops from 24.8 to 21.6 ˚C. Assume that the specific heat and density of the resulting solution are equal to those of water, 4.18 J/(g ˚C) and 1.00 g/mL, respectively and assume that no heat is lost to the calorimeter itself, nor to the surroundings. KCl(s) + H2O(l) --> KCl(aq) ∆H = ? a) Is...
A 9.07-g sample of NaOH is dissolved in 104.9 g of water in a coffee cup...
A 9.07-g sample of NaOH is dissolved in 104.9 g of water in a coffee cup calorimeter. The temperature of the solution rises from 15.49°C to 23.76°C. Calculate ∆Hrxn, in kJ for the dissociation of NaOH in water Assume that the heat capacity for the solution is 4.18 J/g°C.
When 10.0 g KOH is dissolved in 100.0 g of water in a coffee-cup calorimeter, the...
When 10.0 g KOH is dissolved in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 25.18 ˚C to 47.53 ˚C. Calculate the ∆Hrxn for the dissolution process. Assume that the solution has a specific heat capacity of 4.184 J/gK
The salt cesium bromide is soluble in water. When 9.28 g of CsBr is dissolved in...
The salt cesium bromide is soluble in water. When 9.28 g of CsBr is dissolved in 115.00 g of water, the temperature of the solution decreases from 25.00 to 22.72 °C. Based on this observation, calculate the enthalpy of dissolution of CsBr (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. ΔHdissolution =  kJ/mol
A 3.98 g sample of solid NaBr (s) is dissolved in 361 mL of water in...
A 3.98 g sample of solid NaBr (s) is dissolved in 361 mL of water in a coffee cup calorimeter. Once all of the NaBr (s) is dissolved in the water, the final temperature of the solution is found to be 30.04°C. If the initial temperature of the water in the calorimeter was 21.84 °C, calculate the calorimeter constant (in J/K) for the coffee cup calorimeter. The heat of solvation of NaBr (s) is -0.60 kJ/mol.
A 5.80 g sample of solid NH4Br (s) is dissolved in 117 mL of water in...
A 5.80 g sample of solid NH4Br (s) is dissolved in 117 mL of water in a coffee cup calorimeter. Once all of the NH4Br (s) is dissolved in the water, the final temperature of the solution is found to be 6.73°C. If the initial temperature of the water in the calorimeter was 21.63 °C, calculate the calorimeter constant (in J/K) for the coffee cup calorimeter. Report your answer to three significant figures. The heat of solvation of NH4Br (s)...
A 3.56 g sample of solid NH4C2H3O2 (s) is dissolved in 418 mL of water in...
A 3.56 g sample of solid NH4C2H3O2 (s) is dissolved in 418 mL of water in a coffee cup calorimeter. Once all of the NH4C2H3O2 (s) is dissolved in the water, the final temperature of the solution is found to be 24.81°C. If the initial temperature of the water in the calorimeter was 20.81 °C, calculate the calorimeter constant (in J/K) for the coffee cup calorimeter. Report your answer to three significant figures. The heat of solvation of NH4C2H3O2 (s)...
The salt calcium bromide is soluble in water. When 1.48 g of CaBr2 is dissolved in...
The salt calcium bromide is soluble in water. When 1.48 g of CaBr2 is dissolved in 112.00 g of water, the temperature of the solution increases from 25.00 to 26.56 °C. Based on this observation, calculate the enthalpy of dissolution of CaBr2 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. ΔHdissolution =  kJ/mol
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT