Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. this causes sodium azide (nan3) to decompose explosively according to the following reaction: 2nan3 (s) → 2na(s) + 3n2(g) what mass of nan3 must be reacted to inflate an air bag to 70.0 l at stp?

135.2791 g

Explanation:

For STP conditions:

Pressure = 1.00 atm

Temperature = 273.15 K

Volume = 70.0 L

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

1.0 atm × 70.0 L = n × 0.0821 L.atm/K.mol × 273.15 K  

⇒n = 3.1214 moles

Moles of = 3.1214 moles

From the reaction given,

3 moles of Nitrogen gas is formed from 2 moles of sodium azide

1 mole of Nitrogen gas is formed from 2/3 moles of sodium azide

3.1214 moles of Nitrogen gas is formed from (2/3)*3.1214 moles of sodium azide

Moles of sodium azide = 2.0809 moles

Molar mass of sodium azide = 65.0099 g/mol

Mass = Moles * Molar mass = 2.0809 moles * 65.0099 g/mol = 135.2791 g

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.