Question

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.​

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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 6.00-g sample of KSCN is dissolved in water in a calorimeter that has a...
When a 6.00-g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 4.528 kJ·K–1, the temperature decreases by 0.330 K. Calculate the molar heat of solution of KSCN.
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.
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
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.
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 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 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 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
3.00 g of potassium hydroxide (KOH) pellets are put into a constant-pressure calorimeter containing 250 mL...
3.00 g of potassium hydroxide (KOH) pellets are put into a constant-pressure calorimeter containing 250 mL of water. The initial temperature of the water is 22.3°C. The mixture is then stirred until all of the KOH is dissolved. The final temperature of the solution is measured and recorded as 29.7°C. Calculate the heat of solution for potassium hydroxide (ΔHsoln). The specific heat capacity of the solution may be assumed to be the same as that of water since this is...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT