Now calculate the number of moles of H2O:
Molar mass of H2O = 18.02 g/mol
Number of moles = 0.80 g H2O /18.02 g/mol
= 0.044 mol H2O
Given that dH = 1.8 kJ
Molar heat of evaporation = total heat / number of moles
= 1.8 kJ/ 0.044 mol
= 40.9 kJ/mol
Plz help? Conversion of 0 80 g of Iiquid water to steam at 100degreeC rerqures 1...
See Periodic Table See Hir Conversion of 0.802 g of liquid water to steam at 100.0°C requires 1.78 kJ of heat. Calculate the molar enthalpy of evaporation of water at 100.0°C. kJ/mol
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).
Calculate the amount of heat (in kilojoules) required to convert 18.82 g of water to steam at 100° The enthalpy of vaporization for water is 40.79 kJ/mol. ___kJ
How much heat is released when 105 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). A)347 kJ B)54.8 kJ C)319 kJ D)273 kJ
help plz
The first step in ethanol fermentation is the conversion of pyruvic acid to acetaldehyde and carbon dioxide. The process can be simplified to CH3COCOOH) → CH3CHO(C) + CO2(g) Calculate the change in enthalpy for this reaction in kJ using mean bond enthalpies and any other important thermodynamic information supplied on the next to last page of this exam.
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 24.1 g of steam at 158°C is condensed, cooled, and frozen to ice at -50.°C.
23. The enthalpy change for converting 10.0 g of water at 25.0eC to steam at 135.0eC is kJ. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H20, AHius = 6.01 kJ/mol, and AHvap = 40.67 kJ/mol ku. 24. The enthalpy change for converting 1.00 mol of ice at -50.0eC to water at 70.0e is The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K,...
Calculate the amount of energy (in kJ) necessary to convert 557 g of liquid water from 0°C to water vapor at 172°C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g ·°C, and for steam is 1.99 J/g ·°C. (Assume that the specific heat values do not change over the range of temperatures in the problem.) = KJ
calculate the molar heat capacity Cm for water. you knew that 30.1 kJ was required to heat 10.0 g of ice from 0.00 C to steam 100.00 C and that the melting point pin ∆fusH = 6.01 kJ / mol and the evaporating enthalpy ∆vapH = 40.7 kJ / mol.
1.) Determine the enthalpy change when 62.0 g of steam at 135.0 oC is cooled to ice at –15.0 oC. Use the actual enthalpy and heat capacity values 2.) A heater in a hot water tank gives off 30,000 KJ per hour. The initial temperature of 450 kg of water in the tank is 18.0 oC. If the tank is heated for 90 minutes, determine the final temperature of the water. 3.) In general boiling and melting points increase with...