What amount of heat (in kJ) is required to convert 25.8 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g･°C; specific heat capacity of gas = 0.932 J/g･°C; ∆Hvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3°C)

What amount of heat is required to convert 3.30 g of water at 67.0 °C to 3.30 g of steam at 100.0 °C? (heat capacity of water = 4.184 J/g • °C; AHvap = 40.7 kJ/mol) kJ 2 4 5 6. C +/- х 100 3. 1.

What quantity of heat, in kJ, is required to convert 39.0 g of ethanol (C₂H₅OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g • C; ∆Hvap = 39.3 kJ/mol)

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

A sample of steam with a mass of 0.521 g at a temperature of 100 oC condenses into an insulated container holding 4.50 g of water at 5.0 .C. For water, \Delta Hovap = 40.7 kJ/mol and Cwater = 4.18 J/(g-oC). Part A Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer in degrees Celsius to three significant figures.

What quanity of energy does it take to convert 0.451 kg ice at -20.0 degrees celcius to steam at 250.0 degrees celcius? Specific heat capacities: Ice, 2.03J/g degrees celcius; liquid, 4.18 J/g degrees celcius; steam, 2.02 J/g degrees celcius. delta H vap = 40.7kJ/mol; deltaHfus = 6.02kJ/mol

What amount of heat (in kJ) is required to convert 10.8 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g. °C; specific heat capacity of gas = 0.932 J/g⋅ °C; AHvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3 °C)

How much energy will be released by cooling 28.2 grams of steam from 118°C to 37°C?   cice = 2.02 J/g·K; cwater = 4.184 J/g·K; csteam = 1.97 J/g·K; ΔHfusion = 333 J/g; ΔHvap = 2450 J/g

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 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