HomeworkLib
Question

A thermos contains 80.0g of water at 23.4 degrees C. Suppose 0.200 moles of KCl are...

A thermos contains 80.0g of water at 23.4 degrees C. Suppose 0.200 moles of KCl are dissolved in the water. What will be the final temperature of the solution? Assume that there is no energy transfer between the solution and the thermos, and that the specific heat is 4.184J/g*degrees C. Also, the delta H of solvation for KCl at 25 degrees C is 17.1 kJ/mol.

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

thank you vmuch...

0 0
Add a comment
Know the answer?
Add Answer to:
A thermos contains 80.0g of water at 23.4 degrees C. Suppose 0.200 moles of KCl are...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • A .500g sample of KCl is added to 50g of water initially at 25 degrees celsius...

    A .500g sample of KCl is added to 50g of water initially at 25 degrees celsius in a calorimeter. The final temperature of the solution is 23.95 degrees celsius. What is the heat involved in the dissolution of .500g KCl, assuming the heat capacity of the solution is 4.184J/g degrees celsius?

  • A thermos contains 0.200 liters of water that holds 80 ° C, but it should be...

    A thermos contains 0.200 liters of water that holds 80 ° C, but it should be cooled with zero-degree ice. What is the total volume of water when ice is no longer melting? The melting point for ice at 0 ° C is 6.01 kJ mol-1 and the density of the water is 0.9999 g / cm 3 at 0 ° C and 0.9718 g / cm 3 at 80 ° C

  • An insulated Thermos contains 135 g of water at 86.5 ˚C. You put in a 7.06...

    An insulated Thermos contains 135 g of water at 86.5 ˚C. You put in a 7.06 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?

  • An insulated Thermos contains 143 g of water at 82.8 ˚C. You put in a 9.07...

    An insulated Thermos contains 143 g of water at 82.8 ˚C. You put in a 9.07 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?

  • An insulated Thermos contains 116 g of water at 89.5 ˚C. You put in a 7.91...

    An insulated Thermos contains 116 g of water at 89.5 ˚C. You put in a 7.91 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?

  • PLEASE SHOW WORK The standard enthalpy of solution for KCl(s) dissolving in water to form 1...

    PLEASE SHOW WORK The standard enthalpy of solution for KCl(s) dissolving in water to form 1 m solution of aqueous K^+ and Cl^- ions, delta H^0 _soln = +17.2 kJ/mol. Using a coffee calorimeter, 0.15 moles of KCl(s) were dissolved in 150 mL of water. The initial water temperature was 25 C. What would be the final temperature? A 4C B 21 C C 25 C D 29 C E 42.2 C

  • Calculate the final temperature that will be obtained when a 10g portion of KCL is dissolved...

    Calculate the final temperature that will be obtained when a 10g portion of KCL is dissolved in a coffee-cup calorimeter containing 100g of water. Specific heat of the solution is 4.084j/gc delta H sol (KCL)= 17.0kj/mol and initial temperature is 21.0. Assume that density of the solution is 1.00 g/ml and the calorimeter loses only a neglible amount of heat.

  • A .500g sample of KCL is added to 50g of water initially at 25 degrees celsius...

    A .500g sample of KCL is added to 50g of water initially at 25 degrees celsius in a calorimeter. The final temperature of the solution is 23.95 degrees celsius. What is the heat involved per mol of KCL?

  • An insulated Thermos contains 190 cm3 of hot coffee at 87.0°C. You put in a 13.0...

    An insulated Thermos contains 190 cm3 of hot coffee at 87.0°C. You put in a 13.0 g ice cube at its melting point to cool the coffee. By how many degrees has your coffee cooled once the ice has melted and equilibrium is reached? Treat the coffee as though it were pure water and neglect energy exchanges with the environment. The specific heat of water is 4186 J/kg·K. The latent heat of fusion is 333 kJ/kg. The density of water...

  • An insulated Thermos contains 200 cm3 of hot coffee at 80.0°C. You put in a 16.0...

    An insulated Thermos contains 200 cm3 of hot coffee at 80.0°C. You put in a 16.0 g ice cube at its melting point to cool the coffee. By how many degrees has your coffee cooled once the ice has melted and equilibrium is reached? Treat the coffee as though it were pure water and neglect energy exchanges with the environment. The specific heat of water is 4186 J/kg·K. The latent heat of fusion is 333 kJ/kg. The density of water...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT