A 0.551 g sample of steam at 106.1 °C is condensed into a container with 4.66 g of water at 15.2 °C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18 c, the specific heat of steam is g. °C 2.01 , and AH, H vap = -40.7 kJ/mol. Tf = °C

A 0.537 g sample of steam at 103.2 ∘C is condensed into a container with 5.60 g of water at 16.7 ∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18  J g⋅ ∘C,, the specific heat of steam is 2.01  J g⋅ ∘C,, and Δ?vap=40.7 kJ/mol.

How much heat is released( kJ) upon converting one mole of steam (18.0g) from 100 degrees Celsius to water at 25 degree Celsius?

What amount of heat (in kJ) is required to convert 19.1 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g-°C; specific heat capacity of liquid = 1.58 J/g-°C; AHfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)

How much heat energy (in J) is involved when 55 grams of gaseous water, at 107 °C is cooled to 56° C? (Given: ∆Hvap = +40.65 kJ/mol, CH2O(g) = 1.84 J/g°C, CH2O(l) = 4.184 J/g°C). Watch your sign for q!

What amount of heat (in kJ) is required to convert 15.5 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･°C; specific heat capacity of liquid = 1.58 J/g･°C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)

Calculate the heat required to convert 10.0 g of water at 100°C to steam at 100.0 °C. The specific heat of water is 1.00 cal/(g x °C); the heat of fusion is 80.0 cal/g; and the heat of vaporization is 540.0 cal/g.

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

13) Ethanol melts at -114 C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of evaporation is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 and 2.3 J/gK, respectively. How much heat is required to convert 42.0 g of ethanol at 35 °C to the vapor phase at 78 °C?