33.0 mL of water at 38.9 °C is heated to steam at 128.7 °C. Calculate the the total heat (in kJ) required to accomplish this. Cwater=4.18 J/g°C, Csteam = 2.00 J/g°C, Hvap= 40.7 kJ/mol, dH2O = 1.00 g/mI Hint: Draw a heating curve and calculate heat for each segment

Using the information below, calculate how much energy (in kJ) is released when 12.0 g of water vapor at 113.0 ºC is cooled to 100 ºC and then condensed, GFM = 18.016 g/mol. Show all work and report you final answers to the correct units and significant figures. For H2O:  Cs = 2.03 J/(g·°C)     △Hfus = 6.02 kJ/mol                 Cl = 4.18 J/(g·°C)      △Hvap = 40.7 kJ/mol                  Cg = 2.0 J/(g·°C)

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.

A 0.554 g sample of steam at 106.0 °C is condensed into a container with 5.20 g of water at 16.4 °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 2.01 g., and AH vap = 40.7 kJ/mol. T₁ = °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

Some physical properties of water are shown below. melting point boiling point specific heat solid 2.05 J/g °C specfic heat liquid 4.184 J/g.°C specific heat gas 2.02 J/g °C ΔΗ° fusion 6.02 kJ/mol ΔΗ° vaporization 40.7 kJ/mol If 16.6 g of water at 80°C are mixed with 10.7 g of ice at 0.0°C, what is the final temperature of the mixture? °℃ 0.0°C 100.0°C

Which equation calculates the temperature change of 100 g of water that absorbs the same amount of heat as it takes to boil 5 g of water?   Question 12 options:   (100 g / 18 g mol–1 × 40650 J mol–1)  / (5 g × 4.184 J g–1 °C–1)   (5 g / 18 g mol–1 × 40650 J mol–1)  / (100 g × 4.184 J g–1 °C–1)   (100 g × 4.184 J g–1 °C–1)  / (5 g / 18 g mol–1 × 40650 J mol–1)

2. Calculate the amount of energy (in kilojoules) needed to heat 346 g of liquid water from 0°C to 182°C. Assume that the specific heat of water is 4.184 J/gᵒC over the entire liquid range and that the specific heat of steam is 1.99 J/gᵒC. (AHvap = 40.79 kJ/mol for water)

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