1 / 7

Q = ms  T

Calculate the total quantity of heat evolved when 10.0g of steam at 200  C is condensed, cooled , and frozen to ice at -50  C. The specific heat capacity of ice and steam are 2.06J/g  C and 2.03J/g  C respectively. 1. 2. 3. 4. 5. 1. Q = ms  T. Q = (10.0g)(2.03J/g  C)(100  C).

rachel-puckett
Download Presentation

Q = ms  T

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. Calculate the total quantity of heat evolved when 10.0g of steam at 200 C is condensed, cooled , and frozen to ice at -50 C. The specific heat capacity of ice and steam are 2.06J/gC and 2.03J/gC respectively. 1 2 3 4 5

  2. . 1 Q = msT Q = (10.0g)(2.03J/gC)(100C) Q = 2030J = 2.030kJ 1

  3. 2 n(H2O) = mass / molar mass = 10.0g / 18g mol-1 = 0.56 mol H2O vap H (H2O) = 40.6kJ/mol vap H (H2O) = 0.56 mol  40.6 kJ/mol = 22.7 kJ 2

  4. 3 Q = msT Q = (10.0g)(4.18J/gC)(100C) Q = 4180J = 4.180kJ 3

  5. 4 n(H2O) = mass / molar mass = 10.0g / 18g mol-1 = 0.56 mol H2O fus H (H2O) = 40.6kJ/mol fus H (H2O) = 0.56 mol  40.6 kJ/mol = 22.74 kJ 4

  6. 5 Q = msT Q = (10.0g)(2.06J/gC)(50C) Q = 1030J = 1.030kJ 5

  7. Calculate the total quantity of heat evolved when 10.0g of steam at 200 C is condensed, cooled , and frozen to ice at -50 C. Total heat = 2.030kJ + 22.7 kJ + 4.180kJ + 22.74 kJ + 1.030kJ = 52.68kJ

More Related