Calculate the value of Kp for the reaction. Constants| Periodic Table Express yo

Question

Calculate the value of Kp for the reaction. Constants| Periodic Table Express your answer to three significant figures A flask is charged with 1.600 atm of N2O4(g) and 1.00 atm of NO2 (g) at 25 C, and the following equilibrium is achieved N3O4 (g) 2NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.516 atm Submit Previous Answers Request Answer You may want to reference (Pages 639 - 640) Section 15.5 while completing this problem X Incorrect; Try Again; 2 attempts remaining Set up the equilibrium expression for this reaction and use the given equilibrium pressure o the product (0.516 atm) and the equilibrium pressure of the reactant (determined in Part A) to calculate Kp Part C Calculate the value of Kc for the reaction. Express your answer to three significant figures.

Explanation / Answer

Data given.

PN2O4= 1.6 atm

PNO2 = 1atm

In equilibrium:

PN2O4= 1.6 -x

PNO2 = 1 + 2x

and PNO2 = 1 + 2x = 0.516

x = (0.516-1)/2 = -0.242

Then

PN2O4= 1.6 -x = 1.6 - (-0.242) = 1.842 atm

b)

Kp = PNO2^2 / PN2O4 = (0.516) ^2/1.842 = 0.1445

c)

Kp = Kc*(RT)^dn

Kc = Kp / (RT)^dn

Kc = (0.1445)/((.082*298)^(2-1)) = 0.005915

Kc = 0.006

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