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Molecular Formula

Two moles of ...

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Two moles of NH3 gas are introduced into a previously evacuated one litre vessel in which it partially dissociates at high temperature as 2NH3 (g)N2 (g) + 3H2 (g). At equilibrium, onemole of NH3(g) remain. The value of Kc is

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Q. Two moles of

{N H}_{3}

gas are introduced into a previously evacuated one litre vessel in which it partially dissociates at high temperature as

{2 N H}_{3} (g) ⇋ . N_{2} (g) + {3 H}_{2} (g)

. At equilibrium, one mole of

{N H}_{3} (g)

remain. The value of

K_{C}

Q. Two moles of

N H_{3}

are introduced into one litre flask in which it dissociates at high temperature as follows:

2 N H_{3} (g) ⇌ N_{2} (g) + 3 H_{2} (g)

K_{C}

, if at equilibrium

1 m o l e

N H_{3}

Q. Two moles of

N H_{3}

when put into a previously evacuated vessel (one litre), partially dissociate into

N_{2}

H_{2}

. If at equilibrium one mole of

N H_{3}

is present , the equilibrium constant is :

Q. Two moles of ammonia is introduced in a evacuated 500 ml vessel at high temperature. The decomposition reaction is:

{2 N H}_{3} (g) ⇌ N_{2} (g) + {3 H}_{2} (g)

At the equilibrium

{N H}_{3}

becomes 1 mole then the

K_{c}

Q. At a certain temperature (T), the equilibrium constant

(K_{c})

is 1 for the reaction

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

N_{2},

H_{2},

N H_{3}

and 3 moles of inert gas are introduced into a two litre rigid vessel at constant temperature T. It has been found that equilibrium concentration of

H_{2}

N H_{3}

are equal then what is the equilibrium concentration of

N_{2}

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