Calculate the enthalpy chamge when 75.0g of ethanol goes from 87.0 C to -15.0 C, given the following information for ethanol: c ethanol = 2.44j/g*C, Delta Hfusion=5.02 kj/mol, delta Hvap=38.56 kj/mol.
Calculate the enthalpy chamge when 75.0g of ethanol goes from 87.0 C to -15.0 C, given...
Calculate the energy involved (in kJ) when 27.6 g ethanol (CH3CH2OH) goes from 106.5°C to -162.1°C. (Be sure to include the sign.) Ethanol boils at 78.37°C and freezes at -114°C with ΔHvap = 38.56 kJ/mol and ΔHfus = 4.9 kJ/mol; cliquid= 2.440 J/g°C, cgas = 1.699 J/g°C and csolid = 2.419 J/g°C.
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅K are 2.3 J/g⋅K respectively. A) How much heat is required to convert 30.5 g of ethanol at 30 ∘C to the vapor phase at 78 ∘C? Q=______kJ B)How much heat is required to convert 30.5 g of ethanol at -167 ∘C...
How much heat energy is required to convert 15.0 g of solid ethanol at -114.5 °C to gasesous ethanol at 143.1 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45 J/g·°C and that of gaseous ethanol is 1.43 J/g·°C. How much heat energy...
Given the following information for ethanol, C,H,OH (at 1 atm), calculate the amount of heat in kneeded (at 1 atm) to vaporize a 20.6-g sample of liquid ethanol at its normal boiling point of 78.4 °C. boiling point = 78.4 °C AHvap 78.4 °C) = 38.6 kJ/mol melting point = -115°C AH(-115 °C) -5.02 kJ/mol specific heat liquid = 2.46 J/gºC
the normal boiling point of ethanol is 78.3 deg C and its molar enthalpy of vaporization is 38.56 Kj/mol. what is the change in entropy in the system in J/k when 97.2 grams of ethanol at 1 atm condenses to a liquid at the normal boiling point?
Calculate the average molar bond enthalpy of the carbon-hydrogen bond in a CH4 molecule. -- Given that (Delta)Hf [H(g)]= 218.0 kj/mol (Delta)Hf [C(g)]= 716.7 kJ/mol (Delta)Hf [CH4(g)]= -74.6 kJ/mol
UJUH POHL Given the following information: Using the data given below at 25°C, calculate the change in enthalpy (DH) for the following reaction: 2PC13(g) + O2(g) ® 2POC13(g) Calculate the AH°rxn for the combustion of ethanol using the given AH°F. AHºf, ethanol (1) = -277.6 kJ/mol AHºf, water (1) = -285.8 kJ/mol AHºf, carbon dioxide (g) = -393.5 kJ/mol
#14 A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is The bomb had a heat capacity of 540 J/K, and the calorimeter contained 690 g of water. Burning 4.50 g of ethanol, resulted in a rise in temperature from 16.7 °C to 20.6 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184 J/g ⋅ K.) Enthalpy of combustion = _____ kJ/mol
How much energy (in kilojoules) is released when 31.5 g of ethanol vapor at 97.0 ∘C is cooled to -13.5 ∘C? Ethanol has mp = -114.5 ∘C, bp = 78.4 ∘C, ΔHvap = 38.56 kJ/mol and ΔHfusion = 4.60 kJ/mol. The molar heat capacity is 113 J/(K⋅mol) for the liquid and 65.7 J/(K⋅mol) for the vapor.
From the following data, calculate the Enthalpy when Rhombic Sulphur is covered to monoclinic Sulphur S (rhombic) + O2 (gas) -----> SO2 (gas) delta H = -295.1 kJ/mol S (monoclinic) + O2 -------> SO2 (gas) delta H = -296.4 kJ/mol ___________________________________________________ S (rhombic) -------> S (monoclinic) delta H = [x] kJ/mon