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Standard XII

Chemistry

Raoult's Law

NH3 under 1...

Question

$N H_{3}$ under $15$ atm pressure and at $27^{o} C$ is heated to $327^{o} C$ in a closed vessel in the presence of a catalyst. Under these conditions, $N H_{3}$ is partially decomposed and pressure is increased to $25$ atm. The percentage of $N H_{3}$ decomposed is :

30

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50

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67

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75

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Solution

The correct option is B $67$ %
The equilibrium reaction is $2 N H_{3} (g) ⇋ N_{2} (g) + 3 H_{2} (g)$ .
The partial pressures of various species are given in the following table.
$N H_{3}$
$N_{2}$
$H_{2}$
Initial pressure
$15$
$0$
$0$
Change
$- 2 x$
$x$
$3 x$
Equilibrium pressure
$15 - 2 x$
$x$
$3 x$

But, the total pressure at equilibrium is $15 - 2 x + x + 3 x = 25$ or $x = 5$ .
$∴$ Percentage of ammonia decomposed $= \frac{10}{15} \times 100 = 66.67 = 67$ %.

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Similar questions

Ammonia kept under pressure of 15 atm at 27⁰C is heated to 347⁰C in a closed vessel in the presence of catalyst. Under these conditions, NH₃ is partially decomposed according to the equation, $2 N H_{3} ⇋ N_{2} + 3 H_{2}$ . The vessel is such that the volume remains effectively constant whereas pressure increases to 50 atm. Calculate the percentage of NH₃ actually decomposed.

Q. Ammonia under pressure of

15

atm at

27^{o}

C is heated to

347^{o}

C in a closed vessel in the presence of catalyst. Under the conditions,

N H_{3}

is partially decomposed according to the equation,

2 N H_{3} ⇌ N_{2} + 3 H_{2}

. The vessel is such that the volume remains effectively constant whereas pressure increases to

50

atm. Calculate the percentage of actually decomposed.

Q. Ammonia under a pressure of

15

atm at

27^{\circ} C

is heated to

347^{\circ} C

in a closed vessel in the presence of a catalyst. Under the conditions,

N H_{3}

is partially decomposed according to the equation,

2 N H_{3} ⇋ N_{2} + 3 H_{2}

.The vessel is such that the volume remains effectively constant whereas pressure increases to

50 a t m

. Calculate the percentage of

N H_{3}

actually decomposed.

Q. Ammonia at

15

atm and

27^{\circ} C

is heated to

347^{\circ} C

in a closed vessel in the presence of a catalyst. Under the condition,

N H_{3}

is partially decomposed according to the equation,

2 N H_{3} \Leftrightarrow N_{2} + 3 H_{2}

. The vessel is such that the volume remains effectively constant whereas pressure increases to

50

atm. Calculate the percentage of

N H_{3}

actually decomposed.

Ammonia under a pressure of 15 atm at 27⁰C is heated to 347⁰C in a closed vessel in the presence of catalyst. Under the conditions, NH₃ is partially decomposed according to the

equation, 2NH₃N₂+3H₂. The vessel is such that the volume remains

effectively constant whereas pressure increases to 50 atm. Calculate the percentage of NH₃ actually decomposed.

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	$N H_{3}$	$N_{2}$	$H_{2}$
Initial pressure	$15$	$0$	$0$
Change	$- 2 x$	$x$	$3 x$
Equilibrium pressure	$15 - 2 x$	$x$	$3 x$

NH3 under 15 atm pressure and at 27oC is heated to 327oC in a closed vessel in the presence of a catalyst. Under these conditions, NH3 is partially decomposed and pressure is increased to 25 atm. The percentage of NH3 decomposed is :

$N H_{3}$ under $15$ atm pressure and at $27^{o} C$ is heated to $327^{o} C$ in a closed vessel in the presence of a catalyst. Under these conditions, $N H_{3}$ is partially decomposed and pressure is increased to $25$ atm. The percentage of $N H_{3}$ decomposed is :