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E 98% Sun 12:38 PM Q. E Chrome File Edit View History Bookmarks People Window Help Mastering Chemistry: Post Lecture Homework Chapter 15 Adaptive Follow-Up Secure https session.masteringchemistry.co 81720416 m/m Chem 132-02 Help Close c Post Lecture Homework Chapter 15 Adap... Exercise 1 Enhanced with Feedback Resources atm+at e... previous I Item 1 l next Go xercise 15.87 Enhanced with Feedback Sign in Part A At 700 K, CC14 decomposes to carbon and Find the starting pressure of CC4 at this temperature that produces a total pressure of 1.5 atm at chlorine. The Kp for the decomposition is 0.76 equilibrium Express the pressure in atmospheres to three significant figures. You may want to reference (DA pages 674-710) Chapter 15 while completing this problem. Pccuinit atm Submit My Answers Give up Incorrect; Try Again; 5 attempts remaining First, write a balanced chemical equation and set up an ICE (Initial, Change, Equilibrium) table to track the changes to the partial pressures of CCL and C2. (Carbon is a solid, so it does not contribute to pressure.) For example, A can be used to represent the initial pressure of carbon tetrachloride (P init), and -z can be used to represent the change to its partial pressure. When you set up your equilibrium expression, take into account that 1.5atm PT you set up the equilibrium expression correctly, you will need to solve for z using the quadratic formula. Lastly, use the value of z to calculate the initial pressure of CCL. Continue Provide FeedbackExplanation / Answer
Ans -
CCl4 = 2Cl2 + C
preesure of -
pressure Cl2 + pressure CCl4 = 1.5 atm
Cl2 = x
CCl4 = y
x + y = 1.5
kp = x2 / y
0.76 = x2 / y
y = 1.5-x
x2 / 1.5-x = 0.76
x2 + .76x - 1.14 = 0
x = 0.75 and - 1.5
x = 0.75
y = .75
CCl4 <=> C + 2 Cl2
start
?
change
-x .. . . . . .. . +2x
at equilibrium
.75 .. . .. . . .. 0.75
2x = .75
x = .375
initial pressure - .375 = .75
initial pressure = 1.125
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