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Relationship between Vapor Density & Relative Molecular Mass

34 gm of a mi...

Question

34 gm of a mixture containi ng $N_{2}$ and $H_{2}$ in I : 3 by mole is partially converted into $N H_{3}$ . Calculate the vapour density of the mixture (containing remaining $N_{2}$ , $H_{2}$ and $N H_{3}$ after reaction if it has been found that the $N H_{3}$ form required 0.5 moles of $H_{3} P O_{4}$ for complete neutralization.
$3 N H_{3} + H_{3} P O_{4} \to (N H_{4})_{3} P O_{4}$

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Solution

$2 \times$ Vapour density= Mass
$\Rightarrow$ Mass of given sample $(N_{2} + H_{2}) = 34$
$∴$ Vapour density= $\frac{34}{2} = 17$

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34

gm of a mixture containing

N_{2}

H_{2}

1 : 3

by mole is partially converted into

{N H}_{3}

. Calculate the vapour density of the mixture (containing remaining

N_{2}, H_{2}

{N H}_{3}

formed) after reaction if it has been found that the

{N H}_{3}

formed required

0.5

H_{3} {P O}_{4}

for complete neutralization.

Q. If a mixture of

3

H_{2}

and one mole of

N_{2}

is completely converted into

N H_{3}

. What would be the ratio of the initial and final volume at same temperature and pressure?

Q. A mixture containing

2

N_{2}

3

H_{2}

gas is brought to equilibrium in a

3 L

vessel. If the molar concentration of

N H_{3}

at equilibrium is

1 / 3 m o l / L

, calculate the

K_{c}

for the formation of

N H_{3}

.

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

{N H}_{3}

N_{2}

H_{2}

according to the following equation:

{2 N H}_{3} \to N_{2} + {3 H}_{2}

x % o f {N H}_{3}

is converted into product. Rate of diffusion of gaseous mixture is double than that of

{S O}_{2}

under identical conditions. Calculate

x

.

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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