Chemistry Please Help!

Question

Liquid nitroglycerine (C3H5(NO3)3) is a powerful explosive. When it detonates, it produces a gaseous mixture of nitrogen, water, carbon dioxide, and oxygen.

a) What is the theoretical yield of carbon dioxide if 10.00g of the nitroglycerine explodes?

b) If the actual amount of carbon dioxide obtained is 4.81g, what is the percent yield?

c) How many molecules of nitrogen would actually be produced?

Answer 1

4C3H5(NO3)3→6N2+10H2O+12CO2+O2

a)

use molar mass

10g nitro. / 227.11g=0.04403mol nitrog

use coefficients

0.04403mol nitrog * 12molCO2/4mol nitrog = 0.1321 mol CO2

use molar mass

0.1321molCO2(44.01gCO2/1mol)=5.813g CO2

b) %yield=(actual/theoretical)100

%=(4.81/5.813)100

=82.7%

c)

since it's actual, use the actual amount of carbon dioxide from part b, and not theoretical from part a

use molar mass

4.81gCO2(1molCO2/44.01gCO2)=0.1093 mol CO2

use coefficients

0.1093 mol CO2 * (6mol N2/12 mol CO2)=0.0546 mol N2

use avogadro's number (6.02E23=1mol)

0.0546 mol N2 (6.02E23molecules N2/1mol N2)

=3.29E22 molecules N2