1. To heat 18cc of h2o from room temperature to boiling. 2. Then vaporize it. 3....
4) 74 kJ are required to heat 1 cup of water from room temperature to boiling. The wavelength of microwave radiation in a microwave oven is 2.3 x 10-3 m. How many moles of photons are required? 5) Cesium requires a minimum energy of 188 kJ/mol for an electron to be ejected. What is the wavelength of light in nm that possesses the minimum amount of energy needed to cause the electron to eject? 5.4 Balmer-Rydberg 6) Use the Balmer-Rydberg equation to calculate...
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
How much heat is required to vaporize 100.0 g of ethanol, C2H,OH, at its boiling point? The enthalpy of vaporization of ethanol at its boiling point is 38.6 kJ/mol.
How much heat is needed to vaporize 225 g of rubbing alcohol C3H8O at its boiling point? The enthalpy change of vaporization of rubbing alcohol = 0.664 kj/mol.
1. CH MgB 2 HO 1. CH3MOBI 2. HO 1. CHẠMgB 2. HO 1. LiAIHA 2. H2O HCI H2SO MaBr (2 eq) CH3NH2 room temperature heat 200 °C
How much heat is required to vaporize 30.8 g of water at 100 ∘C∘C? (ΔHvap(H2O)=40.7kJ/mol, Heat capacity(H2O)=4.184J/g∘C)(ΔHvap(H2O)=40.7kJ/mol, Heat capacity(H2O)=4.184J/g∘C) Express your answer with the appropriate units.
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) is required to raise the temperature of 141,4 g of ethanol (mw=46,07) from 49.82 °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/gºC, ΔHvap = 48.6 kJ/mol)
How much heat (in kJ) is required to raise the temperature of 288.7 g of ethanol (mw=46.07) from 39.38 °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, ΔHvap = 48.6 kJ/mol)
How much heat (in kJ) is required to raise the temperature of 202.8 g of ethanol (mw=46.07) from 40.34 °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, ΔHvap = 48.6 kJ/mol)