When 8.70 kj of thermal energy is added to 2.50 mol of liquid methanol, it vaporizes....
The normal boiling point of methanol is and the molar enthalpy of vaporization if 71.8 kJ/mol. The value of S when 1.75 mol of vaporizes at 64.7 °C is 0.372 4.24 × 107 372 1.94 × 103 1.
Calculate the amount of heat needed to transform, under standard conditions, 1.0 mol of liquid methanol at 273 K to 1.0 mol of methanol vapor at 373 K. Assume that Cp,m for liquid methanol and for methanol vapor are independent of temperature. (Enthalpy of vaporization of methanol 35.3 KJ/mol-1, Cp,m of methanol 81.6 JK-1/mol)
calculate the change in thermal energy in kJ for a 637 g sample of acetone (molar mass = 58.08 g/mol) to change from -10.3 Celsius to 108 Celsius. given information: enthalpy of fusion: 5.73 kJ/mol enthalpy of vaporization: 31.3 kJ/mol melting point: -94.7 C boiling point: 56.1 C specific heat capacity for solid: 1.65 J/g Celsius specific heat capacity for liquid: 2.16 J/g C specific heat capacity for gas: 1.29 J/g C thank you!!
Up 8. One mole of water at 20° C has 20 kJ of thermal energy added. Calculate the number of moles which remain in the liquid state.
1. Calculate the change in internal energy ΔΕ when 15.6 kJ of heat is added to the system and 1.4 kJ of work is done to the system. 2. How much work can a bicycle pump perform when the the cylinder compresses from 3L to 2.5 L as you apply a pressure of 1.1 atm? J. A hot air baloon expands from 4,00,000L to 4.00,000L by the addion of 130,000000 of eat energy Calculate the change in energy of the...
What amount of thermal energy (in kJ) is required to convert 44.1 g of ethanol at -178 °C completely to gaseous ethanol at 119 °C? The melting point of ethanol is -114 °C and its normal boiling point is 78 °C. The heat of fusion of ethanol is 5.0 kJ mol-1 The heat of vaporization of ethanol at its normal boiling point is 35.0 kJ mol-1 The specific heat capacity of solid ethanol is 1.05 J g-1 °C-1 The specific...
What amount of thermal energy (in kJ) is required to convert 42.0 g of ethanol at -171 °C completely to gaseous ethanol at 99 °C? The melting point of ethanol is -114 °C and its normal boiling point is 78 °C. The heat of fusion of ethanol is 5.0 kJ mol-1 The heat of vaporization of ethanol at its normal boiling point is 35.0 kJ mol-1 The specific heat capacity of solid ethanol is 1.05 J g-1 °C-1 The specific...
The heat of combustion of liquid cumene (C9H12) is -5215.5 kJ/mol at 1 atm and 298 K a) What is the energy of combustion at 1 atm and 298 K? Ecomb = kJ/mol b) Use Thermodynamic Properties to determine its heat of formation. Hf = kJ/mol
1. a. The enthalpy of vaporization of liquid mercury is 59.11 kJ/mol. What quantity of energy as heat is required to vaporize 0.240 mL of mercury at 357 °C, its normal boiling point? The density of mercury is 13.6 g/mL. Energy = ____ kJ b. Determine ethanol’s normal boiling point by slowly changing the temperature to the point where the vapor pressure equals 760 mmHg. What is this temperature? °C
A sample of liquid methanol weighing 5.27 g was burned in a bomb calorimeter at 25°C, and 119.50kJ of heat was evolved. a. Calculate AHº for the combustion of 1 mole of methanol. b. Calculate A/Hºof liquid methanol. A Hºof CO2(g), H2O(g) and H20 (1) are -393.5 kJ/mol, 241.8 kJ/mol, -285.8 kJ/mol, respectively (10 pt)