Question

3&4

QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) 2 Na(s) + 3 N2(g) Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 30.3 L of N2(g) at 25.6 C and 1 00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water 2 H2(g) O2(a)-2 H20(g) How many grams of water could be produced by the reaction of 6.67 liters of hydrogen with 4.11 liters of oxygen at STP? (Hint check for limiting reagent). Click Save and Submit to save and submit. Click Save All Answers to save all answers.

Answer 1

3)

1st find the mol of N2 produced.

Given:

P = 1.0 atm

V = 30.3 L

T = 25.6 oC

= (25.6+273) K

= 298.6 K

find number of moles using:

P * V = n*R*T

1 atm * 30.3 L = n * 0.08206 atm.L/mol.K * 298.6 K

n = 1.237 mol

From given chemical equation,

Mol of NaN3 reacted = (2/3)*mol of N2 produced

= (2/3)*1.237 mol

= 0.825 mol

Molar mass of NaN3,

MM = 1*MM(Na) + 3*MM(N)

= 1*22.99 + 3*14.01

= 65.02 g/mol

use:

mass of NaN3,

m = number of mol * molar mass

= 0.825 mol * 65.02 g/mol

= 53.64 g

Answer: 53.6 g

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