Looking at 2A(g) - B(g): If the initial partial pressure of A is 3.0atm and the

Question

Looking at 2A(g) - B(g): If the initial partial pressure of A is 3.0atm and the initial partial pressure of B is 0atm, what is the value of K if 33% of A has reacted to reach equillibrium?

- this question was from probem 80 in Zumdahl General Chemistry book, chapter 10. In the Chegg solution, a solution was proposed that either I don't understand or is wrong. The chegg solution says that the equillibrium pressure of A is .33(3), but I believe it should be 3-(.33*3), because if 33% reacted, there should be 67% left right?

Explanation / Answer

partial pressure of A = 3(1-2x)

partail pressure of B=2x

where x is the dissociation constant

now if 33% of a has reacted that means x=0.33

Kp=4x^2/3(1-x)=0.2167 atm

Coming to your doubt

Since the initial pressure was 3atm ,equlibrium pressure must be 3(1-2x)=3*0.33=1 atm.Your approach is correct.

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