The relationship between specific heat of a substance and heat gained or lost is as follows:
Here, n is number of moles of the substance.
is the heat vaporization of the substance.
Heat vaporization is of a substance is the amount of heat required to vaporize one mole of the substance.
Calculate the number of moles of water as follows:
Now, calculate the heat energy absorbed to boil the water at atmospheric pressure is as follows:
Therefore, the total heat absorbed is .
Ans:The heat energy absorbed is .
the heat of vaporization of water is 40.66 kJ/mol. How much heat is absorbed when 2.88...
< Question 11 of 18 > The heat of vaporization of water is 40.66 kJ/mol. How much heat is absorbed when 1.87 g of water boils at atmospheric pressure? heat:
R55150 < Question 21 of 22 > The heat of vaporization of water is 40.66 kJ/mol. How much heat is absorbed when 3.17 g of water boils at atmospheric pressure? heat: about us Careers privacy policy terms of use contact us help
The heat of vaporization of water at 100°C is 40.66 kJ/mol. Calculate the quantity of heat that is absorbed/released when 5.00 g of steam condenses to liquid water at 100°C. 147 kJ of heat are absorbed. 147 kJ of heat are released. 11.3 kJ of heat are absorbed 11.3 kJ of heat are released.
the heat of vaporization of water at 100*c is 40.66 kj/mol. calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100*c
The heat of vaporization of water at 100°C is 46.06 kJ/mol. Calculate the quantity of heat that is absorbed/released when 90.0 g of steam condenses to liquid water at 100°C. 203 kJ of heat are absorbed. 20.3 kJ of heat are released. 230.3 kJ of heat are released. 203.3 kJ of heat are released.
Calculate the heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100°C. DHvap(water) = 40.66 kJ/mol.
The heat of vaporization of CH_2CI_2 is 28.0 kJ/mol. Calculate the entropy the entropy change when 42 g of CH_2CI_2 boils at its boiling point of 39.8degreeC. 17 J/K 44J/K 59J/K 350J/K 700J/K
The Standard enthalpy of vaporization of water at 100.0 oC is 40.66 KJ*mol-1. The Cp,m values for the liquid and the vapor water are, respectively, 75.3 and 33.58 J*K-1*mol-1. Assume that the heat capacities are independent of temperature, and that the vapor behaves as an ideal gas. a) Calculate sys in taking one mole of liquid water at 25.0 oC and 1.00 atm to gaseous water at 95.0 oC and 0.500 atm. b) Assume that the temperature and pressure of...
How much heat (in kJ) is released when 125.0 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol ∙ °C), and the molar heat capacity of ice is 36.4 J/(mol ∙ °C).
The heat of vaporization AH, of ethyl aceae4Hs 35.1 kJ/mol. Calculate the change in entropy AS when 4.6 g of ethyl acetate boils at Be sure your answer contains a unit symbol. Round your answer to 2 significant digits