What amount of heat (in kJ) is required to convert 10.1 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)

Liquid butane is used in cigarette lighters. The boiling point of butane at 1 atm pressure is -1.0 °C and its ∆H(vap) is 22.44 kJ/mol. R = 8.314 ×10⁻³ kJ/mol･K. Calculate the pressure (in atm) of the butane in the lighter at 19.5 °C.

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.

Sulfur dioxide is produced in enormous amounts for sulfuric acid production. It melts at −73.0 ° C and boils at −10.0 ° C. Its  Δ H o   fus  is 8.619 kJ/mol, and its  Δ H o   vap  is 25.73 kJ/mol. The specific heat capacities of the liquid and gas are 0.995 J/g  ·  K and 0.622 J/g  ·  K, respectively. How much heat is required to convert 7.750 kg of solid SO2 at the melting point to a gas at 60.0 ° C?

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)

A 25.5-g sample of ice at -10.0°C is mixed with 110.0 g water at 85.0°C. Calculate the final temperature (in °C) of the mixture assuming no heat loss to the surroundings. The heat capacities for H₂O(l) and H₂O(s) are 4.184 J/g･°C and 2.03 J/g･°C, respectively, and the enthalpy of fusion of ice is 6.02 kJ/mol.

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