The following information is given for ethanol, C₂H5OH, at 1atm: AHvap (78.4 °C) = 38.6 kJ/mol boiling point = 78.4 °C specific heat liquid = 2.46 J/g °C At a pressure of 1 atm, kJ of heat are needed to vaporize a 39.5 g sample of liquid ethanol at its normal boiling point of 78.4 °C.

Converting a 5.00 g sample of liquid cyclohexane (C6H₁2) at 30.7 °C to vapor at 140.7 °C requires kJ of heat. molar mass = 84.16 g/mol melting point = 6.5 °C boiling point = 80.7 °C AHfus = 2.68 kJ/mol AHvap = 32.0 kJ/mol Csolid 1.2 J/g °C Cliquid 2.8 J/g °C Cgas = 0.90 J/g °C

Calculate the energy released as heat when 18.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg(1) Constants for mercury at 1 atm melting point enthalpy of fusion 28.0 J/(mol-K) # 234.32 K 2.29 kJ/mol 9 = MacBook Pro

Calculate the heat required to convert 22.2 g of propyl alcohol, C3H3O, from a solid at -141°C into the gaseous state at 115°C. The normal melting and boiling points of this substance are -127°C and 97°C, respectively. The heat of fusion is 86.2 J/g, and the heat of vaporization is 694 J/g. The specific heats of the solid, liquid and gaseous states are, respectively, 2.36, 2.83 and 1.76 J/g/K.

Ethanol (C₂H₂OH) meits 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 and 2.3 J/(g-K), respectively. Y Part A How much heat is required to convert 30.5 g of ethanol at 28 °C to the vapor phase at 78 "C? Express your answer in kilojoules to three significant figures. 195] ΑΣΦ Submit Part 8 Request Answer Submit ? How much heat is required to convert 30.5 g of ethanol at-160 C to the vapor phase at 78 "C7 Express your answer in kilojoules to two significant figures. VA24 Request Answer kJ kJ

The following information is given for cobalt at 1atm: boiling point = 3097°C AHvap = 6.60 kJ/g melting point = 1495°C AHfus = 263 J/g What is the energy change, Q, in kJ for the process of freezing a 39.8 g sample of liquid cobalt at its normal melting point of 1495°C. kJ

Ethanol (C2 H5 OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -125 °C to liquid ethanol at -50 °C? 3949 207.3 6.67 8.97 -12.5

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

What quantity of heat, in kJ, is required to convert 12.0 g of ethanol (C₂H₂OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g C; AHvap = 39.3 kJ/mol) ●