USEFUL DATA: Specific heat (solid): 0.40 J/g•K Heat of fusion: 6.11 J/g Specific heat (liquid): 0.65 J/g•K Heat of vaporization: 281.4 J/g Specific heat (gas): 0.32 J/g•K 46. Estimate the boiling point (K) of NOOK if it requires 160,486 J to completely transform 113 grams of liquid NOOK at 508 K to vapor at its boiling point. Round off your answer to the nearest whole number and place your answer on the space provided.

USEFUL DATA: Specific heat (solid): 0.40 J/g•K Heat of fusion: 6.11 J/g Specific heat (liquid): 0.65 J/g•K Heat of vaporization: 281.4 J/g Specific heat (gas): 0.32 J/g•K 46. Estimate the boiling point (K) of NOOK if it requires 160,486 J to completely transform 113 grams of liquid NOOK at 508 K to vapor at its boiling point. Round off your answer to the nearest whole number and place your answer on the space provided.

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

Chemistry
What quantity of heat (in J) would be required to convert 6.91 mol of a pure substance from a liquid at 40.0 °C to a gas at 113.0 °C? + Cliquid = 1.45 J/mol °C Tboiling = 88.5 °C Cgas = 0.65 J/mol•°C AHvaporization = 1.23 kJ/mol
How much heat energy is required to boil 23.0 g of ammonia, NH,? The molar heat of vaporization of ammonia is 23.4 kJ/mol. kJ = b
The following information is given for aluminum at latm: boiling point = 2467 °C AHvap(2467 °C) = 284 kJ/mol melting point = 660 °C AHfug(660 °C) = 10.8 kJ/mol specific heat solid= 0.900 J/g°C specific heat liquid = 1.09 J/g°C What is AH in kJ for the process of freezing a 26.3 g sample of liquid aluminum at its normal melting point of 660 °C. kJ
Which of the following equations represents the correct heat of formation of water vapour? O H2(g) + ½ 02(g) --> H2O(1) H2(g) + O(g) --> H2O(g) 2H(g) + O(g) –->; H2O(g) H2(g) + O2(g) –-> 2H2O(g) H2(g) + /½ O2(g) --> H2O(g)
What quantity of heat is required to convert 19.0 g of ethanol (C₂H₅OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (heat capacity of ethanol = 2.46 J/g • C; ∆Hvap = 39.3 kJ/mol)
Two 20.0 g ice cubes at -17.0 °C are placed into 235 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/ (mol·K) heat capacity of H,O(1) 75.3 J/ (mol·K) T = enthalpy of fusion of H,O 6.01 kJ/mol
How much heat energy is required to convert 65.6 g of solid iron at 27 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/(g- °C). q= kJ
Some physical properties of water are shown below. melting point boiling point specific heat solid 2.05 J/g °C specfic heat liquid 4.184 J/g.°C specific heat gas 2.02 J/g °C ΔΗ° fusion 6.02 kJ/mol ΔΗ° vaporization 40.7 kJ/mol If 16.6 g of water at 80°C are mixed with 10.7 g of ice at 0.0°C, what is the final temperature of the mixture? °℃ 0.0°C 100.0°C
Determine the normal boiling point of a liquid with vapor pressure 63.8 mmHg at 64.50°C, given that its molar heat of vaporization is 43.5 kJ/mol.
Using the following data for water, determine the energy required to melt 1.00 mole of ice (solid water) at its melting point. Boiling point Melting point Enthalpy of vaporization 2,260 J/g Enthalpy of fusion Specific heat capacity (solid) Specific heat capacity (liquid) Specific heat capacity (gas) 373 K 273 K 334 J/g 2.11 J/(g· K) 4.18 J/(g· K) 2.08 J/(g· K) Select one: a. 6.02 kJ b. 23.2 kJ c. 2.26 kJ d. 11.7 kJ e. 4.96 kJ
A substance has the following properties: AHfus 10.0 kJ/mol AHvap=20.0 kJ/mol Cp (solid) = 60. J mol-¹ K-¹ Cp (liquid) = 30. J mol-¹ K-¹ Cp (gas) = 60. J mol-¹ K-¹ =