Calculate the amount of heat released (in kilojoules) when 68.0 g of steam at 124°C is converted to asolid at a solid at 20° Assume Cs of H2O (s) is 2.09 J/g °C, 4.184 J/g °C over the entire liquid range andC, steam is 1.99 J/g °C, AHmelting = 6.01 kJ/mol and AHvap = 40.67 kJ/mol (Remember AH is a statefunction)-2840 kJ-3047 kJ+3047 kJ-3.047 kJ2.840 kJ+2840 kJ

Given information:- Mass of steam = 68.0 g- Initial temperature of steam = 124°C- Final temperature…

Answered: Calculate the amount of heat released…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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What amount of heat, in kJ, is required to convert 3.90 g of water at 67.0 °C to 3.90 g of steam at 100.0 °C? (specific heat capacity of water = 4.184 J/g • °C; ∆Hvap = 40.7 kJ/mol)
The following information is given for n-pentane, C5H12, at 1atm: AHvap(36.2 °C) = 25.8 kJ/mol boiling point specific heat liquid = 36.2 °C = 2.28 J/g °C At a pressure of 1 atm, normal boiling point of 36.2 °C. kJ of heat are needed to vaporize a 25.5 g sample of liquid n-pentane at its
How much energy is needed to turn 10.0 g of water at 25°C to steam ( = 6.01 kJ/mol; = 40.76 kJ/mol; c = 75.3 J/mol • °C)?
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8.) AHvap is a way to measure intermolecular forces quantitatively. Calculate the amount of energy (in kilojoules) needed to cool 550 g of water vapor from 150°C to -20°C. Assume that the specific heat of water is 4.184 J/g °C over the entire liquid range and the specific heat of steam is 1.99 J/g °C. The AHvap for water is 40.79 kJ/mol. The AHfus 6.01 kJ/mol. The specific heat of ice is 2.01 J/g °C
Substance C has a normal boiling point of 89.3 ºC, and an enthalpy of vaporization of 31.3 kJ/mol. How many kilojoules of heat is required to change 3.675 mol of C from a liquid at 89.3 ºC to a gas at 89.3 ºC?
Suppose that 0.87 gg of water condenses on a 85.0 gg block of iron that is initially at 20 °C.C. If the heat released during condensation goes only to warming the iron block, what is the final temperature (in oC) of the iron block? (Assume a constant enthalpy of vaporization for water of 44.0 kJ/mol and a heat capacity for iron of 0.449 J/(g-oC).) Express your answer in degrees Celsius to two significant figures.
calculate the total amount of heat needed to convert 22.50 g of solid carbon tetrachloride, CCl4 at a temperature of -35 C to vapor form at 120 C, given the following values for CCl4 : melting point= -22.9 C; boiling point = 76.2C; change in H fusion = 2.69 kj/mol ; change in H vapor =29.8 kj/mol
The following information is given for benzene, C6H6, at 1atm: AHvap(80.1 °C) = 30.7 kJ/mol boiling point = 80.1 °C specific heat liquid = 1.74 J/g°C At a pressure of 1 atm, boiling point of 80.1 °C. kJ of heat are needed to vaporize a 40.2 g sample of liquid benzene at its normal
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