Ethanol melts at -144°C and boils at 78°C. The enthalpy of fusion of ethanol is 5.02 kJ per mole and its enthalpy of vaporization is 38.56 kj/mol the specific heats of solid and liquid 0.97J/g•K and 2.3 J/ g•K. How much heat is required to convert 9.02 g of ethanol at - 141ﾟC to the vapor phase at 78ﾟC.

Please explain step by step (it would be helpful if you also graph it)

13) Ethanol melts at -114 C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of evaporation is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 and 2.3 J/gK, respectively. How much heat is required to convert 42.0 g of ethanol at 35 °C to the vapor phase at 78 °C?

What is the vapor pressure of ethanol (in mmHg) at 52.7°C if its vapor pressure is 400.0 mmHg at 63.5°C? (AHvap = 39.3 kJ/mol; R = 8.314 J/K • mol) %3D

What is the vapor pressure of ethanol in (mmHg) at 62.5°C if it's vapor pressure is 400.0 mmHq at 63,5°c? | AH vap= =99.3 KJ/mol; R= 8.314 S/kimoi>

Which equation calculates the heat of vaporization of water when it takes the same amount of heat to boil 5 g of water as it does to heat 100 g of water by 27°C?   Question 11 options:   (100 g × 4.184 J g–1 °C–1 × 27°C)  / (5 g / 18 g mol–1)   (5 g × 4.184 J g–1 °C–1 × 27°C)  / (100 g / 18 g mol–1)   (5 g / 18 g mol–1) / (100 g × 4.184 J g–1 °C–1 × 27°C)

Consider the following data for an unknown substance X: AHvap 19.00 kJ/mol Specific heat capacity of liquid = 2.10 J/g °C Boiling point = 66.0°C Molar mass = 119.0 g/mol When the temperature of 1.000 mole of X(g) is lowered from 91.0°C to form X(1) at 41.0°C, 30.38 kJ of heat is released. Calculate the specific heat сараcity of X(g). Specific heat capacity = J/g °C Submit Answer Try Another Version 10 item attempts remaining 11 33°F 12 Tch

calculate the total amount of heat needed to convert 22.50 g of solid carbon tetrachloride, CCl4 at a temperature of -35 C to vapor form at 120 C, given the following values for CCl4 : melting point= -22.9 C; boiling point = 76.2C; change in H fusion = 2.69 kj/mol ; change in H vapor =29.8 kj/mol

The following information is given for benzene, C6H6, at 1atm: AHvap(80.1 °C) = 30.7 kJ/mol boiling point = 80.1 °C specific heat liquid = 1.74 J/g°C At a pressure of 1 atm, boiling point of 80.1 °C. kJ of heat are needed to vaporize a 40.2 g sample of liquid benzene at its normal

Chloroform, CHCl3 is a volatile liquid and has a boiling point of 61.7 ° C and has a heat of vaporization of 31.4 kJ/mol. What is the vapor pressure of chloroform at 37.2 °C?