What amount of heat, in kJ, is required to vaporize 198.00 g of ethanol (C2H5OH)? (AHvap = 43.3 kJ/mol) %3D

Liquid butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 35.5 g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol. Show your work.

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

Ethanol (C2H5OH) melts at -114 oC and boils at 78 oC. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 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 is required to convert 20.18 g of ethanol at -220 oC to the vapor phase at 78 oC? (Give your answer in unit of kilojoules)

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Calculate the heat required to bring 10.0 g CCl2F2 from -29.8°C as a liquid to the gas phase at 10.0°C. (molar mass = 120.91 g/mol) Cs (gas) = 0.074 kJ/mol·K ΔHvap = 20.1 kJ/mol ΔHfus = 4.14 kJ/mol

Enter your answer in the provided box. From the data below, calculate the total heat (in J) needed to convert 0.821 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 Cgas: 1.43 J/g °C AHⓇ : 40.5 kJ/mol vap Cliquid 2.45 J/g.°C

A sample of C3H4Br2 has a normal boiling temperature of 131.5 °C. The enthalpy of vaporization for this compound is 35.4 kJ/mol. How much energy would be required to heat a 13.5 gram sample of liquid C3H4Br2 from 97.5 °C to a gas at 187.2 °C? The specific heat for the liquid is 0.865 J/g °C and the specific heat for the gas is 0.364 J/g. °C.

A 0.527 g sample of steam at 103.7 °C is condensed into a container with 5.86 g of water at 16.1 °C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18 , the specific heat of steam is g. C 2.01 , and AH vap = -40.7 kJ/mol. g. °C Tf = °C