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The main reason that distillation is a costly method for purifying water is the high energy required to heat and vaporize water. • Part A Using the density, specific heat, and heat of vaporization of water from Agpendix B in the textbook, calculate the amount of energy required to vaporize 1.00 gal of water beginning with water at 25 °C. Express your answer using two significant figures. E= 9700 kJ Submit Previous AnswerS v Correct The volume of the water, given in gallons, must first be converted to grams using the density from the appendix. 3780 gal x 1qt xIL x 1000 ml. x 0.99707 E H,O – 1.43 x 107 e H,O 1 gal X 1.057 gt X 1ml. First, the water needs to be heated from 25 °C to 100 °C. The heat associated with this process is calculated using the specific heat of water from the appendix. 9 - MCAT = 1.43 x 107 g H,0 x 4.184J x (100°C – 25°C) x TE 1000 J - 4.481 x 10° kJ Once the water reaches 100 °C. it must then be vaporized. The heat associated with this process is then calculated using the heat of vaporization from the appendix. 1 mol H,0 40.67 kJ a = 1.43 x 10" g H20 x TR02 H,0 X mol H,0 = 3.223 x 107 kJ The total amount of energy required is the sum of these two heat values. 4.481 x 10° kJ + 3.223 x 10° kJ 9700 kJ /gal H,O • Part B If the energy is provided by electricity costing $0.087 /kwh. calculate its cost. (1 kwh = 3.6 x 10° J) Express your answer using two significant figures. VoAEd ? $ 44.93 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining

The main reason that distillation is a costly method for purifying water is the high energy required to heat and vaporize water. • Part A Using the density, specific heat, and heat of vaporization of water from Agpendix B in the textbook, calculate the amount of energy required to vaporize 1.00 gal of water beginning with water at 25 °C. Express your answer using two significant figures. E= 9700 kJ Submit Previous AnswerS v Correct The volume of the water, given in gallons, must first be converted to grams using the density from the appendix. 3780 gal x 1qt xIL x 1000 ml. x 0.99707 E H,O – 1.43 x 107 e H,O 1 gal X 1.057 gt X 1ml. First, the water needs to be heated from 25 °C to 100 °C. The heat associated with this process is calculated using the specific heat of water from the appendix. 9 - MCAT = 1.43 x 107 g H,0 x 4.184J x (100°C – 25°C) x TE 1000 J - 4.481 x 10° kJ Once the water reaches 100 °C. it must then be vaporized. The heat associated with this process is then calculated using the heat of vaporization from the appendix. 1 mol H,0 40.67 kJ a = 1.43 x 10" g H20 x TR02 H,0 X mol H,0 = 3.223 x 107 kJ The total amount of energy required is the sum of these two heat values. 4.481 x 10° kJ + 3.223 x 10° kJ 9700 kJ /gal H,O • Part B If the energy is provided by electricity costing $0.087 /kwh. calculate its cost. (1 kwh = 3.6 x 10° J) Express your answer using two significant figures. VoAEd ? $ 44.93 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The main reason that distillation is a costly method for purifying water is the high energy required to heat and vaporize water. Part A Using the density, specific heat, and heat of vaporization of water from Appendix B in the textbook, calculate the amount of energy required to vaporize 1.00 gal of water beginning with water at 25 °C. Express your answer using two significant figures. E = 9700 kJ Submit Previous Answers v Correct The volume of the water, given in gallons, must first be converted to grams using the density from the appendix. 3780 gal x t x1L x 1000 mL. x 0.99707 g H20 – 1.43 x 107 g H.O 1L 4 qt 1 gal 1.43 x 107 g H20 1.057 qt 1 ml. First, the water needs to be heated from 25 °C to 100 °C. The heat associated with this process is calculated using the specific heat of water from the appendix. = mcAT = 1.43 x 107 g H,O x 9 4.184 J g.°C x (100°C – 25°C) x I kJ * 1000 J %3D = 4.481 x 106 k.J Once the water reaches 100 °C, it must then be vaporized. The heat associated with this process is then calculated using the heat of vaporization from the appendix. 9 = 1.43 x 107 g H,0 x - 1 mol H0 18.02 g H,0 40.67 k.J mol H,0 = 3.223 x 107 kJ The total amount of energy required is the sum of these two heat values. energy 4.481 x 10° k.J + 3.223 x 10° kJ = 9700 kJ/gal H,0 Part B If the energy is provided by electricity costing S0.087 /kwh, calculate its cost. (1 kwh = 3.6 x 10 J) Express your answer using two significant figures. ? $ 44.93 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining
Transcribed Image Text:The main reason that distillation is a costly method for purifying water is the high energy required to heat and vaporize water. Part A Using the density, specific heat, and heat of vaporization of water from Appendix B in the textbook, calculate the amount of energy required to vaporize 1.00 gal of water beginning with water at 25 °C. Express your answer using two significant figures. E = 9700 kJ Submit Previous Answers v Correct The volume of the water, given in gallons, must first be converted to grams using the density from the appendix. 3780 gal x t x1L x 1000 mL. x 0.99707 g H20 – 1.43 x 107 g H.O 1L 4 qt 1 gal 1.43 x 107 g H20 1.057 qt 1 ml. First, the water needs to be heated from 25 °C to 100 °C. The heat associated with this process is calculated using the specific heat of water from the appendix. = mcAT = 1.43 x 107 g H,O x 9 4.184 J g.°C x (100°C – 25°C) x I kJ * 1000 J %3D = 4.481 x 106 k.J Once the water reaches 100 °C, it must then be vaporized. The heat associated with this process is then calculated using the heat of vaporization from the appendix. 9 = 1.43 x 107 g H,0 x - 1 mol H0 18.02 g H,0 40.67 k.J mol H,0 = 3.223 x 107 kJ The total amount of energy required is the sum of these two heat values. energy 4.481 x 10° k.J + 3.223 x 10° kJ = 9700 kJ/gal H,0 Part B If the energy is provided by electricity costing S0.087 /kwh, calculate its cost. (1 kwh = 3.6 x 10 J) Express your answer using two significant figures. ? $ 44.93 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining
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