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Characteristics of Equilibrium Constant

A nitrogen-hy...

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A nitrogen-hydrogen mixture initially in the molar ratio of 1:3 reached equilibrium to from ammonia when 25% of the N2 and H2 had reacted .If the pressure of the system was 21 atm , the partial pressure of ammonia at the equilibrium was

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Q. In a closed container, nitrogen and hydrogen mixture initially in a mole ratio of 1:4 reached equilibrium is found that the half hydrogen is converted to ammonia. If the original pressure was 180 atm, what will be the partial pressure of ammonia at equilibrium (there is no change in temperature)?

Q. If a mixture of

N_{2}

H_{2}

in the ratio 1 : 3 at 50 atmosphere and

650^{o} C

is allowed to react till equilibrium is reached. Ammonia present at equilibrium was at 25 atm pressure. Calculate the equilibrium constant (

K_{P}

) for the reaction.

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

Q. If a mixture of

N_{2}

H_{2}

in the ratio 1 : 3 at 50 atmosphere and

650^{o} C

is allowed to react till equilibrium is reached. Ammonia present at equilibrium was at 25 atm pressure. Calculate the equilibrium constant (

K_{P}

) for the reaction.

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

Q. For the reaction

N_{2} + 3 H_{2} ⇌ 2 N H_{3},

N_{2} : H_{2}

were taken in the ratio of 1 : 3. Up to the point of equilibrium 50% each reactant has been reacted. If total pressure at equilibrium is P. The partial pressure of ammonia would be -

Q. A mixture of Nitrogen and Hydrogen is at an initial pressure of

200 a t m

20 %

of the mixture reacts by the times equilibrium is reached, the equilibrium pressure of the mixture is:

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