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Calculate partial pressure of B at equil...

Calculate partial pressure of B at equilibrium in the following equilibrium
`A(s) iff B(g) +2C(g), " " K_(P)=32 atm^(3)`.

A

2

B

3

C

17

D

5.8

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The correct Answer is:
A
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Knowledge Check

  • Calculate partial pressure of B at equilibrium in the following equilibrium A(s)hArrB(g)+2C(g),K_(p)=32atm^(3).

    A
    2
    B
    3
    C
    17
    D
    5.8

  • Consider the reaction N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g) The equilibrium constant of the above reaction is K_(p) If pure ammonia is left to dissociated, the partial pressure of ammonia at equilibrium is given by : (Assume that P_(NH_(3)) lt lt P_(total) at equilibrium)

    A
    `3^(3//2)K_(p)^(1//2)P^(2)/16`
    B
    `3^(3//2)K_(p)^(1//2)P^(2)/4`
    C
    `K_(p)^(1//2)P^(2)/16`
    D
    `K_(p)^(1//2)P^(2)/4`

  • Two equilibria are simultaneously existing in a vessel at 25^(@)C NO(g)+NO_(2)(g)hArrN_(2)O_(3)(g)K_(P_(1)) 2NO_(2)(g) hArrN_(2)O_(4)(g)K_(P_(2))=8 atm^(-1) Initially only NO(g) and NO_(2)(g) are present in 3:5 mole ratio. The total pressure at equilibrium is 5.5 atm and the partial pressure of NO_(2) at equilibrium is 0.5 atm The incorrect statement(s) regarding the above equilibria is/are

    A
    `K_(P_(1))` for the equilibrium is `0.4 atm^(-1)`
    B
    Partial pressure of `N_(2)O_(4)` at equilibrium is `1.6 atm`
    C
    Partial pressure of `N_(2)O_(3)` at equilibrium is `2atm`
    D
    Partial pressure of `NO` at equilibrium is `2.5 atm`
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