1 / 19

69 Days Until the Final!

69 Days Until the Final!. Catalyst: If you have 2000 g of water and you heat it up from 10 o C to 70 o C, then what is the total heat produced in this process? The specific heat of water is 4.18 J/(g x o C). If 980,000 J of energy are added to 6200 g of water at 291 K, what will the

chloe-foley
Download Presentation

69 Days Until the Final!

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. 69 Days Until the Final! • Catalyst: • If you have 2000 g of water and you heat it up from 10 oC to 70 oC, then what is the total heat produced in this process? The specific heat of water is 4.18 J/(g x oC). • If 980,000 J of energy are added to 6200 g of water at 291 K, what will the final temperature of the water be? The specific heat of water is 4.18 J/(g x oC) End

  2. Would you Rather…

  3. Justify – TPS • Why did you choose the choice that you did? Why do you think it would be better to be burned by one then the other?

  4. Today’s Learning Target • 7.7 – I can use the latent heat of phase change to calculate the amount of energy that is released or absorbed during a change of phase.

  5. ΔHfusion and ΔHvaporization • There is a large amount of energy that is required to change a solid into a liquid and a liquid into a gas (and vice versa) • ΔHfusion = Energy to change solid to a liquid. • ΔHvaporization = Energy to change liquid to a gas. • ΔHfreezing = Energy to change liquid to a solid • ΔHcondensation = Energy to change gas to a liquid

  6. Latent Heat • We can calculate the amount of energy that is necessary to convert a substance from one phase to another • Latent Heat – The energy absorbed as a substance changes phases

  7. ΔH of vaporization/condensation Latent Heats ΔH of fusion/freezing

  8. Equation for Latent Heat • m = mass of compound • ΔH = Enthalpy values for phase changes (constants)

  9. Class Example • You have a 2000 kg of ethanol. Calculate the energy you would need to turn solid aluminum into liquid. The ΔHfusion is 109 kJ/kg.

  10. Table Talk • You have 6342 kg of mercury. How much energy would be required to take mercury from liquid to a gas? The ΔHvaporization is 294 kJ/kg

  11. Stop and Jot • You have an ice cube of H2O that weighs 2000 kg and you melt it to liquid. How much energy does that require? The ΔHfusion is 334 kJ/kg.

  12. Summarize

  13. Connect 4

  14. Work Time • Begin working on your “Homework 7.3” • There will be an exit slip after this activity

  15. Learning Log Assessment Rate yourself 1 – 4 on LTs 7.7

  16. Exit Slip 1. You have 2000 g of water that is heated from 25 C to 100 C. What is the heat absorbed by this process. The specific heat of water is 4.184 J/(gxC)

  17. Learning Log Assessment Using your exit slip score, re-rate yourself on LTs 7.7

  18. Closing Time • Test Tuesday!

More Related