Chemistry calculation help

Question

1 Does temperature make a difference in how much carbon dioxide gas is needed to inflate a 60-L air bag using the reaction of sodium bicarbonate and acetic acid? Compare a winter day at 0°C and standard pressure with a summer day at 35°C and standard pressure. Calculate the number of moles of carbon dioxide gas required for a 60-L inflation at both temperatures and then calculate the percent difference in moles.

Winter Day at 0°C:

Summer Day at 35°C:

2 Calculate the number of moles of nitrogen gas (N2) that are needed to inflate a 67-L driver-side air bag at standard temperature (0°C) and pressure (1 atm). Start by balancing the reaction shown below.

_NaN3(s) ----> _Na(s) + _N2(g)

3 Calculate the grams of sodium azide (NaN3) required to produce the number of moles of nitrogen gas calculated in Question 2.

4 How many grams of sodium metal are produced in the decomposition of sodium azide shown in Question 2?

Answer 1

1). Yes, the temperature will make a difference.

Winter day @ 0ºC (273K) and standard pressure of 1 atm:

PV = nRT

n = PV/RT

n = (1 atm)(60 L) / (0.0821 Latm/Kmol)(273K)

n = 2.68 mols CO₂ needed

Summer day @ 35ºC (308K) and standard pressure of 1 atm:

PV = nRT

n = PV/RT

n = (1 atm)(60 L) / (0.0821)(308K)

n = 2.37 mols CO₂ needed

Percent difference in mols needed = 2.68 - 2.37 / 2.68 (x100%) = 11.6% difference

2). 2NaN₃(s) ----> 2Na(s) + 3N₂(g) ... balanced equation

PV = nRT

n = PV/RT = (1 atm)(67 L) / (0.0821 Latm/Kmol)(273K)

n = 2.99 mols N2 needed

3). mass of NaN₃ needed = 2.99 mols N₂ x 2 mols NaN₃ / 3 mols N₂ x 65.0 g NaN₃/mol = 130 g NaN₃ (2 s.f.)

4). mass Na produced = 2.99 mols N₂ x 2 mols Na / 3 mols N₂ x 23 g Na/mol = 46 g Na (2 sig. figs.)