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LiRa [457]
3 years ago
5

Air-bags can be inflated by the decomposition of sodium azide, NaN3. At 25.0◦C and 1.10 atm, what volume of N2(g) is produced by

the decomposition of 71.4 g NaN3 under the following chemical reaction: 2NaN3(s) → 2Na(l) + 3N2(g)
Chemistry
1 answer:
Mashcka [7]3 years ago
4 0

Answer:

V = 36.7L of N_{2}

Explanation:

1. Write the chemical reaction for the decomposition of sodium azide:

_{2}NaN_{3}(l)=_{2}Na(s)+_{3}N_{2}(g)

2. Find the number of moles of N_{2} produced by the decomposition of 71.4g of NaN_{3}:

71.4gNaN_{3}*\frac{1molNaN_{3}}{65gNaN_{3}}*\frac{3molesN_{2}}{2molesNaN_{3}}=1.65molesN_{2}

3. Use the ideal gas equation to find the Volume of N_{2} occupied by 1.65 moles of N_{2}, at the temperature and pressure given by the problem:

PV=nRT

Solving for V:

V=\frac{nRT}{P}

Converting the temperature from ◦C to K:

25◦C+273.15=298.15K

Replacing values:

V=\frac{1.65mol*(0.082\frac{atm.L}{mol.K})*298.15K}{1.10atm}

V=36.7L of N_{2}

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