14. Calculate how many Joules of energy would be required to change 32.9 g of water at 35°C to steam at 120°C. You will need to break this problem into four steps. a) Find the Joules needed to heat the water to the boiling point. (8938.9 J) b) Find the Joules needed to vaporize the water. (74,354 J) c) Find the Joules needed to heat the vapor (steam) from the boiling point to 120°C. (1329 J) d) Add your answers to steps a, b, and c. (84,622 J)

14. Calculate how many Joules of energy would be required to change 32.9 g of water at 35°C to steam at 120°C. You will need to break this problem into four steps. a) Find the Joules needed to heat the water to the boiling point. (8938.9 J) b) Find the Joules needed to vaporize the water. (74,354 J) c) Find the Joules needed to heat the vapor (steam) from the boiling point to 120°C. (1329 J) d) Add your answers to steps a, b, and c. (84,622 J)

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...

See similar textbooks

Similar questions

Energy Constants for H2O334 J/g = Heat of Fusion (Hf)2260 J/g = Heat of Vaporization (Hv)2.11 J/goC = Specific Heat Capacity of solid water4.18 J/goC = Specific Heat Capacity of liquid water2.00 =J/goC = Specific Heat Capacity of water vapor3. A 12-oz can of soft drink (m = 340 g) at 25oC is placed in a cooler where the temperature is 0oC. How much energy must be removed from the soft drink for it to become ice at 0oC?
Which produces more heat?Os(s) ⟶ 2O2(g) ⟶ OsO4(s)orOs(s) ⟶ 2O2(g) ⟶ OsO4(g)for the phase change OsO4(s) ⟶ OsO4(g) ΔH = 56.4 kJ
The specific heat capacity of lead is 0.13 J/g∙oC. How much heat (in J) is required to raise the temperature of 278 g of lead from 20 oC to 50 oC? a) 1.1 x 103 b) 5.8 x 10-4 c) 2.0 d) 0.13
What change in energy is required to heat 55.00 g of water at 15.00 0C to vapor at 180.0 0C?
How many kilojoules of heat are absorbed when 24.0 g CH4(g) is produced at constant pressure? (CH4: 16.04 g/mol) 2CH3OH(g) --->2CH4(g) + O2(g) /\H = +252.8 kJ
4
Ethylene glycol (specific heat 2.42 J/g°C) is used as a coolant in automotive engines. Calculate the energy released (q) when 3.65 kg of ethylene glycol is cooled from 132 °C to 85 °C.
17. When 420 Joules of heat energy is added to 10. grams of water at 20.°C, the final temperature of the water will be (3) 40.°C (4) 100°C (1) 10.°C (2) 30.°C
Please fill in the four blanks. Thank you!
How much energy must be absorbed by 20.0 g of water to increase its temperature from283.0 °C to 303.0 °C? (Cp of H2O = 4.184 J/g°C)
49 a b с D to A 124.1 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C 147.6 °C. (heat capacity of liquid = 1.62 J/g °C; heat capacity of gas = 1.04 J/g °C; AHvap = 78.11 kJ/mol; normal boiling point, Tb = 160.3 °C) How much energy (in kJ) is absorbed/released to cool the gas? How much energy (in kJ) is absorbed/released to condense the gas? How much energy (in kJ) is absorbed/released to cool the liquid? A What is the total amount of energy that must be absorbed/released for the entire process?
Damp clothes can prove fatal when the outdoor temperature drops (e.g. death by hypothermia). If the clothes you are wearing absorb 94.2 g of water and then dry in a cold wind on Optimist Hill, how much heat (in kJ) would your body lose during the process? (Co H20 = 75.3 J/mol°C and AHvap.H20= 40.81 kJ/mol) (Answer to 1 decimal place) Type your answer.. Next Previous