Question

Nitro glycerine is used as an explosive. The equation for the explosive reaction is
$4C_3\underset{\left(l\right)}{H_5}\left(\right(N{O}_3){)}_3\to \underset{\left(g\right)}{12C{O}_2}+\underset{\left(l\right)}{10H_{2}O}+\underset{\left(g\right)}{6N_2}+\underset{\left(g\right)}{O_2}$
(Atomic mass of $C=12,H=1,N=14,O=16)$
i) How many moles does the equation show for i) Nitroglycerine ii) gas molecules produced?
ii) How many moles of gas molecules are obtained from $1$ mole of nitroglycerine?
iii) What is the mass of $1$ mole of nitroglycerine?

Answer 1

Given :$4C_3\underset{\left(l\right)}{H_5}\left(\right(N{O}_3){)}_3\to \underset{\left(g\right)}{12C{O}_2}+\underset{\left(l\right)}{10H_{2}O}+\underset{\left(g\right)}{6N_2}+\underset{\left(g\right)}{O_2}$

$i.$ The number of moles of nitroglycerine $=4moles.$

The number of gas molecules $=12+6+1=19moles$.

$ii.$ $4$ moles of nitroglycerine gives $19$ moles of gas molecules.

Hence, $14$ mole of nitroglycerine gives $=\frac{14}{19}=4.75$ moles of gas molecules.

$iii.$ Mass of $1$$moleof$C_3H_5{(NO_3)}_3\\ =36+5+186\\=227g$