For the following endothermic equilibrium established by dissociation of $$NH_{ 4 }HS$$ to its components::

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On decomposition of

N H_{4} H S

, the following equilibrium is established.

N H_{4} H S ⇌ N H_{3} (g) + H_{2} S (g)

If the total pressure is

P

atm, then the equilibrium constant

K_{P}

is equal to:

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solid NH4HS(s) dissociates to give NH3(g) and H2 (G) and is allowed to attain equilibrium at 100 c . if the value of Kp for its dissociation is found to be 0.34 , find the total pressure at equillibrium and partial pressure of each component

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On decomposition of

N H_{4} H S,

the following equilibrium is established :

N H_{4} H S (s) ⇌ N H_{3} (g) + H_{2} S (g)

If the total pressure is P atm, then the equilibrium constant

K_{P}

is equal to:

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HI was heated in a sealed tube at

440^{o} C

till the equilibrium was established. The dissociation of HI was found to be 22%. According to following reaction,

2 H I ⇌ H_{2} + I_{2}

. The equilibrium constant for dissociation is -

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21. Ammonium hydrogen sulphide dissociate as follows NH4HS(s) <=>NH3(g)+H2S(g), if solid NH4HS is placed in an evacuated flask at certain temperature it will dissociate until the total pressure is 600 torr. (a) calculate the value of equilibrium constant for the dissociation reaction. (b) additional NH3 is introduced into the equilibrium mixture without changing the temperature until partial pressure of NH3 is 750 torr, what is the partial pressure of H2S under these conditions? What is the total pressure in the flask?

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