From the data below, calculate the total heat (in J) needed to convert 0.442 mol of gaseous ethanol at 300.0°C and 1 atm to liquid ethanol at 25.0°C and 1 atm: b.p. at
1 atm: 78.5°C
ΔH o vap : 40.5 kJ/mol
cgas: 1.43 J/g·°C
cliquid: 2.45 J/g·°C
From the data below, calculate the total heat (in J) needed to convert 0.442 mol of...
From the data below, calculate the total heat (in J) needed to convert 0.100 mol of gaseous ethanol at 300.0°C and 1 atm to liquid ethanol at 25.0°C and 1 atm: b.p. at 1 atm: 78.5°C AH : 40.5 kJ/mol vap Cliquid: 2.45 J/g °C Cgas: 1.43 J/g.°C
Enter your answer in the provided box. From the data below, calculate the total heat (in J) needed to convert 0.172 mol of gaseous ethanol at 300.0°C and 1 atm to liquid ethanol at 25.0°C and 1 atm: AH 40.5 kJ/mol b.p. at 1 atm: 78.5°C vap Cliquid 2.45 J/goC 1.43 J/goC Cgas Enter your answer in the provided box. From the data below, calculate the total heat (in J) needed to convert 0.172 mol of gaseous ethanol at 300.0°C...
From the data below, calculate the total heat (in J) needed to convert 0.670 mol of gaseous ethanol at 300.0 C and 1 atm to liquid ethanol at 25.0 C and 1 atm: b.p. at 1 atm: 78.5 C H vap: 40.5 kJ/mol c ethanol( g ): 1.43 J/g *C c ethanol( l ): 2.45 J/g *C
My answer is wrong for the 6th time what am I doing wrong and how do i do this Enter your answer in the provided box. From the data below, calculate the total heat (in J) needed to convert 0.803 mol of gaseous ethanol at 300.0°C and 1 atm to liquid ethanol at 25.0°C and 1 atm: b.p. at 1 atm: 78.5°C AH®: 40.5 kJ/mol vap Cgas: 1.43 J/g.°C Cliquid: 2.45 J/g °C -4849|o1 J
From the data below, calculate the total heat (in J) needed to convert 20.00 g of ice at −8.50°C to liquid water at 0.600°C: m.p. at 1 atm: 0.0°C ΔH o fus : 6.02 kJ/mol c liquid: 4.184 J/g·°C. c solid: 2.09 J/g·°C
From the data below, calculate the total heat (in J) needed to convert 15.00 g of ice at −8.75°C to liquid water at 0.650°C: m.p. at 1 atm: 0.0°C ΔH o fus : 6.02 kJ/mol c liquid: 4.184 J/g·°C csolid: 2.09 J/g·°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...
Determine the amount of heat required to convert 500.0 g of liquid ethanol at 25.0°C into gaseous ethanol at 125°C. Use the following information on ethanol (C2H5OH) to calculate the amount of heat for each of the steps. Melting Point = −117°C Boiling Point = 78.3°C Molar Heat Capacities: Csolid =113 J/mol °C Cliquid = 420 J/mol °C ΔHfusion = 5.02 kJ/molΔHvaporization = 39.3 kJ/mol
How much heat energy is required to convert 82.0 g of solid ethanol at -114.5 degree C to gaseous ethanol at 167.4 degree 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 degree C and a normal boiling point of 78.4 degree C. The specific heat capacity of liquid ethanol is 2.45 J/g middot degree C and that of gaseous ethanol...
How much heat energy is required to convert 16.2 g of solid ethanol at -114.5 °C to gasesous ethanol at 191.9 °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.