Liquid butane (C4H10) has a higher heating value of 43,789 KJ/kg at 298 K and enthalpy of vaporization of 363 kJ/kg. Calculate the enthalpy of formation for butane vapour at 298 K. Show all the calculation steps.
Liquid butane (C4H10) has a higher heating value of 43,789 KJ/kg at 298 K and enthalpy...
The standard enthalpy of combustion of butane is -2878 kJ/mol at 298 K. Calculate the standard enthalpy of formation of butane at 298 K.
Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a normal boiling point of -0.4 ∘C. A 250 mL sealed flask contains 0.7 g of butane at −22∘C. How much butane is present as a liquid at −22∘C? Express your answer using two significant figures. If the butane is warmed to 25 ∘C, how much liquid butane is present?
Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a normal boiling point of -0.4 C. A 250 mL sealed flask contains 0.5 g of butane at -22 C. How much butane is present as a liquid? If the butane is warmed to 25 C, how much is present as a liquid?
The vapor pressure of liquid C4H10 is 324.1 mmHg at a temperature of 251.0 K. The enthalpy of vaporization, ΔHvap, for this liquid is 22.4 kJ/mol. What is the vapor pressure of C4H10 at a temperature of 269.2 K, in mmHg?
Calculate the higher heating value in kJ/mand kJ/kg at 10 °C and 3 atm for an LPG gas mixture 60% propane and 40% butane
The standard enthalpy of combustion of cyclopropane is -2091 kJ/mol at 298 K. The enthalpy of formation of CO_2 (g) and H_2 O (I) are -393 kJ/mol and -286 kJ/mol, respectively. Calculate the enthalpy of formation of cyclopropane Given that the enthalpy of formation of propene is 20.42 kJ/mol, please calculate the enthalpy of isomerization of cyclopropane to propene.
Determine the higher heating value of methyl alcohol (CH_3 OH) given that its enthalpy of formation is -238 000 kj/kg-mol. Assume that the gasoline at the pumps is a mixture of 90% octane and 10% methyl alcohol, determine the mixtures heating value.
(a) Explain the difference between the enthalpy of formation of liquid and gaseous water,-286 and - 242 kJ/mol, respectively, at 298 K. b) Explain why the enthalpy of vaporization of water at 100 oC (40.7 kJ/mol) is lower than at 25 oC (44 kJ/mol)
3. A liquid compound has an enthalpy of vaporization equal to 65.0 kJ and an entropy of equal to 98 J/K at its boiling point. Calculate the boiling point of the compound. AH = 65 kJ AS - 987
1) The enthalpy of vaporization for a liquid is found to be 14.4 kJ mol- at 180 K, its normal boiling point. The molar volumes of the liquid and the vapour at the boiling point are are 115 mL mol-1, and 14.5 L mol-1, respectively. a) Use the Clapeyron equation to estimage the temperature dependence of the vapour pressure (dp/dT) at the normal boiling point. b) Use the Clausius-Clapeyron equation to estimate dp/dT. c) Does the Clausius-Clapeyron equation overestimate or...