Question

Nitroglycerin (c3h5n3o9) is a powerful explosive. its decomposition may be represented by 4c3h5n3o9 → 6n2 12co2 10h2o o2 this reaction generates a large amount of heat and gaseous products. it is the sudden formation of these gases, together with their rapid expansion, that produces the explosion. (a) what is the maximum amount of o2 in grams that can be obtained from 4.50 × 102 g of nitroglycerin

Answer 1

The balanced chemical reaction describing this decomposition is as follows:
4c3h5n3o9 .............> 6N2 + 12CO2 +10H2O + O2

From the periodic table:
mass of oxygen = 16 grams
mass of nitrogen = 14 grams
mass of hydrogen = 1 gram
mass of carbon = 12 grams
Therefore:
mass of C3H5N3O9 = 3(12) + 5(1) + 3(14) + 9(16) = 227 grams
mass of O2 = 2(16) = 32 grams

From the balanced chemical equation:
4(227) = 908 grams of C3H5N3O9 produce 32 grams of O2. Therefore, to know the amount of oxygen produced from 4.5*10^2 grams C3H5N3O9, all we need to do is cross multiplication as follows:
amount of oxygen = (4.5*10^2*32) / (908) = 15.859 grams

Answer 2

Answer:

15.8528 grams of oxygen will be obtained.

Explanation:

$4C_3H_5N_3O_9\rightarrow 6N_2+12CO_2+10H_2O+O_2$

Mass of nitroglycerin = $4.50\times 10^{2} g$

Moles of nitroglycerin:

$\frac{4.50\times 10^{2} g}{227.08 g/mol}=1.9816 mol$

According to reaction, 4 moles of nitroglycerin gives 1 mole of oxygen gas.

then 1.9816 mol of nitroglycerin will give:

$\frac{1}{4}\times 1.9816=0.4954$ moles of oxygen gas.

Mass of oxygen ;

$0.4954 mol\times 32 g/mol=15.8528 g$

15.8528 grams of oxygen will be obtained.