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Standard XII

Chemistry

Gay Lussac's Law, Avagadro's Law

Automobile ai...

Question

Automobile airbags are inflated with $N_{2}$ gas which is formed by the decomposition of solid sodium azide $(N a N_{3})$ . The other product is Na $-$ metal. Calculate the volume of $N_{2}$ gas at $27^{\circ} C$ and 756 Torr formed by the decomposing of 125 gm of sodium azide:

71.4 L

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61.4 L

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51.4 L

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41.4 L

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Solution

The correct option is B 71.4 L
$2 N a N_{3} ⇌ 2 N a + 3 N_{2}$
The number of moles of sodium azide are $\frac{125}{65} = 1.923$ .
The number of moles of nitrogen are $1.923 \times \frac{3}{2} = 2.885$ .
The volume of nitrogen is $V = \frac{n R T}{P} = \frac{2.885 \times 0.0821 \times 300 \times 760}{750} = 71.4 L$

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Similar questions

Q. Automobile air bags are inflated with

N_{2}

gas which is formed by the decomposition of solid sodium azide

({N a N}_{3})

. The other product is

N a -

metal. Calculate the volume of

N_{2}

gas at

27

and 1 atm formed by the decomposing of 130gm of sodium azide.

Q. Sodium azide

(N a N_{3})

is an explosive chemical used in automobile airbags. It is made by the following reaction:

N a N O_{3} + 3 N a N H_{2} \to N a N_{3} + 3 N a O H + N H_{3}

One takes 17.0 g of

N a N O_{3}

and 13.0 g of

N a N H_{2}

. If this amount is used in automobile bags, how much

N_{2}

is formed due to collision at STP?

Q. Sodium azide

(N a N_{3})

is an explosive chemical used in automobile airbags. It is made by the following reaction:

N a N O_{3} + 3 N a N H_{2} \to N a N_{3} + 3 N a O H + N H_{3}

One takes 17.0 g of

N a N O_{3}

and 13.0 g of

N a N H_{2}

. If this amount is used in automobile bags, how much

N_{2}

is formed due to collision at STP?

Q. Sodium azide, the explosive chemical used in automobile airbags is made by the following reaction:

N a N O_{3} + 3 N a N H_{2} ⟶ N a N_{3} + 3 N a O H + N H_{3}

If you combine

15.0 g N a N O_{3}

with

15.0 g N a N H_{2}

, what mass of

N a N_{3}

is produced? (Round to the nearest integer)

Q. Dissociation of sodium azide is given by,

N a N_{3} \to N a + 3 / 2 N_{2}

Δ H

for this is__________.

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Automobile airbags are inflated with N2 gas which is formed by the decomposition of solid sodium azide (NaN3). The other product is Na − metal. Calculate the volume of N2 gas at 27∘C and 756 Torr formed by the decomposing of 125 gm of sodium azide:

The correct option is B 71.4 L2NaN3⇌2Na+3N2The number of moles of sodium azide are 12565=1.923.The number of moles of nitrogen are 1.923×32=2.885.The volume of nitrogen is V=nRTP=2.885×0.0821×300×760750=71.4L

Automobile airbags are inflated with $N_{2}$ gas which is formed by the decomposition of solid sodium azide $(N a N_{3})$ . The other product is Na $-$ metal. Calculate the volume of $N_{2}$ gas at $27^{\circ} C$ and 756 Torr formed by the decomposing of 125 gm of sodium azide: