Student Solutions Manual for Ball's Physical Chemistry, 2nd
2nd Edition
ISBN: 9798214169019
Author: David W. Ball
Publisher: Cengage Learning US
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Textbook Question
Chapter 1, Problem 1.15E
A 2.0 L soda bottle is pressurized with 4.5 atm of CO2 at 298 K. If the temperature is increased to 317 K, what is the pressure of the CO2?
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Consider the reaction:
2 NO(g) + Br2(g) =2 NOBr(g)
A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br2) into a
sealed 1.00 L reaction vessel and then allowed the reaction to reach
equilibrium.
The pressure of the NOBR at equilibrium at 25.0°C is 0.444 bar. (R =
0.08314 L·bar/mol· K and MW of Br2 is 159.808 g/mol.)
Calculate the Kp.
Incorrect, 1 attempt remaining
Your submission:
Feedback:
Use PV=nRT to determine the initial
pressures of the reactants. You can
then determine the pressures of the
reactants equilibrium by subtracting
the pressure that reacted. Kp =
P(NOBr)*/P(NO)²*P(Br)2
43.8
%3D
Consider the reaction:
2 NO(g) + Br2(g) =2 NOBI(g)
A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br2) into a
sealed 1.00 L reaction vessel and then allowed the reaction to reach
equilibrium.
The pressure of the NOBR at equilibrium at 25.0°C is 0.444 bar. (R =
0.08314 L·bar/mol·K and MW of Br2 is 159.808 g/mol.)
Calculate the Kp.
Please work out question #4 completely. I need to see the steps and how the equations are set up.
Chapter 1 Solutions
Student Solutions Manual for Ball's Physical Chemistry, 2nd
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY