Question 15 of 20 Submit The enthalpy for boiling water is 40.7 kJ/mol. How much heat...
Question 5 How much heat (in kJ) is required to evaporate 1.54 mol of acetone at the boiling point the values from the CH122 Equation Sheet for this question) 1 pts Question 6 What mass of ice (ing) can be melted if 8.42 kJ of thermal energy are added at the freezing point? Use molar mass = 18.02 g/mol D Question 5 1 pts How much heat (in kJ) is required to evaporate 1.54 mol of acetone at the boiling...
a. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g of liquid ethanol from -5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid= 2.46J/g°C AHvap=38.6 kJ/mol b. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g water from 5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid=4.184 /g°C AHvap=40.7 kJ/mol
The heat of vaporization of water at 373 K is 40.7 kJ/mol Part A Find for the evaporation of 471 g of water at this temperature. Express your answer with the appropriate units. HAO ? 9= 999 Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Find to for the evaporation of 471 g of water at this temperature. Express your answer with the appropriate units.
The enthalpy of formation of water is -241.8 kJ/mol. How much heat is released when 7g of hydrogen reacts with excess oxygen to form water?
Knowing that delta H of water is 40.7 Kj/mol How many KJ will be required to vaporize 50.0 g of water? Calculate the percent error if you obtain a value of 39.2 Kj/mol for delta h vap for water for experiment
D Question 5 1 pts How much heat (in kJ) is required to evaporate 1.54 mol of acetone at the boiling point? (use the values from the CH122 Equation Sheet for this question) Question 6 1 pts What mass of ice (ing) can be melted if 8.42 kJ of thermal energy are added at the freezing point? Use molar mass = 18.02 g/mol Question 7 1 pts Cancier the heatine rury of a substance in the image below. Moving from...
A pot of water with 251 g of water is boiling. At 100oC how much energy (in kJ) will need to be added until all of the water converts to steam? ΔHvap = 40.7 kJ/mol
QUESTION 3 How much heat (in kJ) is required to raise the temperature of 122 g of ethanol (mw 46.07) from 11.29 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat - 2.46 J/g°C, AHyap = 48.6 kJ/mol) QUESTION 4 What is the change in enthalpy (in kJ) when 40.1 g of ethanol (mw-46.07) is condensed at its boiling temperature? (specific heat 2.46 J/g°C, AHvap 48.6 kJ/mol)...
How much heat in kJ gets rid of condensing 7.13 g of water vapor at 100 ° C and then cools the water formed to 25 ° C? [ΔHvap = 40.7 kJ / mol at 100 ° C and the natural heat of water c (H2O (l)) = 4.18 J g-1 ° C-1] Note. look up the units in the calculations and give the answer in kJ
water has a molar heat capacity of 75.38 J/(mol 12. Water has a molar heat capacity of 75.38 J/(mol x °C) and its vaporization enthalpy at 100°C is 40.7 kJ/mol. How much energy is needed to convert 36 g liquid H20 at 70.0°C to steam at 100°C? A) 85.9 kJ B) 126 kJ C) 77.6 kJ D) 81.4 kJ E) 45.2 kJ