The following information is given for n-pentane, C5H12, at 1atm:boiling point = 36.2 °Cspecific heat liquid = 2.28 3/9°CAHvap(36.2 °C) = 25.8 kJ/molAt a pressure of 1 atm, what is AH in kJ for the process of condensing a 38.1 g sample of gaseous n-pentane at itsnormal boiling point of 36.2 °C.kj

Given:Molar enthalpy of vaporization at 36.2°C: ΔHvap = 25.8 kJ/molSpecific heat of liquid…

Answered: The following information is given for…

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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Solid cesium bromate dissolves in water according to the equation below. CsBrO3 (s)→ Cs+ (aq) + BrO3(aq) AH° +50.46 kJ/mol 10.00 grams of solid CsBrO3 dissolves in 46.0 grams of water initially at a temperature of 30.00 °C in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter. [You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g.°C)] Tfinal Check °℃ =
Assuming no phase transition, what is the change in temperature (°C) if 310.0 mL ethanol (molar mass 46.08 g/mol) absorbs 4.50 kJ of heat? The density of ethanol is 0.789 g/mL and the molar heat capacity of ethanol is 109.5 J/mol·°C. | °C 1 2 3 4 C 7 8 9. +/- х 100
An aluminum can of mass 0.14kg contains water at 17.5°C. Iron pellets with a total mass of 6.3kg at 85.1°C are dropped into the can, and the can and it's contents come to equilibrium af 32.9°C. Specific heat of water = 4190 J/(kg•°C). Specific heat of aluminum = 910 J/(kg•°C). Specific heat of iron = 470 J/(kg•°C). how many kilograms of water are in the can? (3 sig fig)
A 130.9 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C. (heat capacity of liquid = 1.62 J/g. °C; heat capacity of gas = 1.04 J/g∙ °C; AHvap = 78.11 kJ/mol; normal boiling point, Tb = 160.3 °C) How much energy (in kJ) is absorbed/released to cool the gas? +
The following information is given for benzene, CáHá, at 1atm: AHvap(80.1 °C) = 30.7 kJ/mol boiling point 80.1 °C specific heat liquid = KJ 1.74 J/g °C At a pressure of 1 atm, what is AH in kJ for the process of condensing a 47.4 g sample of gaseous benzene at its normal boiling point of 80.1 °C.
1 " A 47.0 g sample of aluminum, which has a specific heat capacity of 0.897 J.g •°C is dropped into an insulated container containing 150.0 g of water at 20.0 °C and a constant pressure of 1 atm. The initial temperature of the aluminum is 95.0 °C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits. °C x10 X
Butane, C4H10, is vaporized at its boiling point. C4H10(1) → C4H10(g) AH° = 301.5 kJ/mol, ASº = 761.4 J/mol·K Calculate the boiling point temperature (in K) at standard conditions.

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