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Standard XII

Chemistry

Heat of Reaction

The dissociat...

Question

The dissociation pressure of solid ammonium hydro-sulphide at $27^{\circ} C$ is $60 c m$ . What will be the total pressure when it dissociates at the same temperature in presence of $N H_{3}$ at a pressure of $45 c m$ ? Assume $N H_{4} H S$ dissociates completely into $N H_{3}$ and $H_{2} S$ .

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Solution

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

$N H_{3}$
$H_{2} S$ Total pressure
Partial pressures (cm) during first decomposition
30
30
60
Partial pressures (cm) during second decomposition
45
30
75
Hence, the total pressure after second decomposition will be 75 cm.

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Similar questions

Q. Ammonium hydrogen sulphide dissociates as follows

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

If solid

N H_{4} H S

is placed in an evacuated flask at certain temperature it will dissociate until the total is

600 t o r r

.
(a) Calculate the value of equilibrium constant for the dissociation reaction.
(b) Additional

N H_{3}

is until introduced into the equilibrium mixture without changing the temperature until partial pressure of

N H_{3}

750 t o r r

, what is the partial pressure of

H_{2} S

under these conditions? What is the total pressure in the flask?

Q. Ammonium hydrogen sulphide dissociates as follows

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

If solid

N H_{4} H S

is placed in an evacuated flask at certain temperature it will dissociate until the total pressure is

600

torr.
a) Calculate the value of equillibrium constant for the dissociation reaction
b) Addional

N H_{3}

is introduced into the equillibrium mixture without changing the temperature until partial pressure of

N H_{3}

750

torr, what is the partial pressure of

H_{2} S

under these conditions? What is the total pressure in the flask?

Q. An amount of solid

N H_{4} H S

is placed in a flask already containing ammonia gas at a certain temperature at

0.50 a t m

pressure. Ammonium hydrogen sulphide decomposed to yield

N H_{3}

and

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gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to

0.84 a t m

. The equilibrium constant for

N H_{4} H S

decomposition at this temperature is:

Q. A flask containing 0.50 atm of ammonia contains some solid

N H_{4} H S

which undergoes dissociation according to

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

Calculate the pressure of

N H_{3}

and

H_{2} S

at equilibrium

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Also calculate the total pressure.

Q. Solid Ammonium carbamate dissociates as:

N H_{2} C O O N H_{4} (s) ⇌ 2 N H_{3} (g) + C O_{2} (g) .

In a closed vessel solid ammonium carbamate is in equilibrium with its dissociation products. At equilibrium, ammonia is added such that the partial pressure of

N H_{3}

at new equilibrium now equals the original total pressure.

Calculate the ratio of total pressure at new equilibrium to that of original total pressure.

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	$N H_{3}$	$H_{2} S$	Total pressure
Partial pressures (cm) during first decomposition	30	30	60
Partial pressures (cm) during second decomposition	45	30	75

The dissociation pressure of solid ammonium hydro-sulphide at 27∘C is 60 cm. What will be the total pressure when it dissociates at the same temperature in presence of NH3 at a pressure of 45 cm? Assume NH4HS dissociates completely into NH3 and H2S.

NH4(s)⇌NH3(g)+H2S(g)NH3H2STotal pressurePartial pressures (cm) during first decomposition 303060Partial pressures (cm) during second decomposition453075Hence, the total pressure after second decomposition will be 75 cm.

The dissociation pressure of solid ammonium hydro-sulphide at $27^{\circ} C$ is $60 c m$ . What will be the total pressure when it dissociates at the same temperature in presence of $N H_{3}$ at a pressure of $45 c m$ ? Assume $N H_{4} H S$ dissociates completely into $N H_{3}$ and $H_{2} S$ .

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

$N H_{3}$
$H_{2} S$ Total pressure
Partial pressures (cm) during first decomposition
30
30
60
Partial pressures (cm) during second decomposition
45
30
75
Hence, the total pressure after second decomposition will be 75 cm.