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Hi asked in Science & MathematicsChemistry · 8 years ago

How do you calculate the Kp of these reactions?

For the reaction H2(g) + Br2(g) <=> 2HBr(g), Kp = 3.5 x 10^4 at 1495 K. What is the value of Kp for the reaction, HBr(g) <=> ½ H2(g) + ½ Br2(g)?

Whenever I do it out I get 2.9 x 10^-5.

The answer sheet says the answer is 5.3 x 10-3

Update:

5.3 x 10^-3 is the answer, not 5.3 x 10-3. I still can't figure out why.

1 Answer

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  • Rais
    Lv 6
    8 years ago
    Favorite Answer

    H2(g) + Br2(g) <=> 2HBr(g), Kp = 3.5 x 10^4 = [HBr]^2/{[H2]x[Br2]}

    HBr(g) <=> ½ H2(g) + ½ Br2(g)

    K'p = [H2]^1/2 x [Br2]^1/2/[HBr]

    OR K'p^2 = [H2] x [Br2]/[HBr]^2 (Making square of both sides)

    OR K'p^2 = 1/Kp = 1/(3.5x10^4) = 0.2857x10^-4

    OR K'p = SQRT (0.2857x10^-4) = 0.5345 x 10^-2 = 5.3 x 10^-3

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