Question

35. Ammonium perchlorate, NH CO., is a common fuel component of solid fuel rockets. If 75% of the oxygen in NH.CO. was converted to molecular oxygen, how many grams of molecular oxygen would be produced from 117.5 kg ammonium perchlorate? (atomic weights in amu: N = 14.01, CI = 35.45, 0 = 16.00, H = 1.008) a. 4.8 x 10^g 02 b. 6.4 x 10^g 02 C. 2.2 x 10^g 02 d. 2.4 x 10^g 02

Answer 1

Answer: The mass of molecular oxygen produced is $4.8\times 10^4g$

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$      .....(1)

Given mass of ammonium perchlorate = 117.5 kg = 117500 g     (Conversion factor:  1 kg = 1000 g)  

Molar mass of ammonium perchlorate = 117.5 g/mol

Putting values in equation 1, we get:

$\text{Moles of ammonium perchlorate}=\frac{117500g}{117.5g/mol}=1000mol$

The chemical equation for the decomposition of ammonium perchlorate follows:

$2NH_4ClO_4\rightarrow 2NH_3+2HClO+3O_2$

By Stoichiometry of the reaction:

2 moles of ammonium perchlorate produces 3 moles of molecular oxygen

So, 1000 moles of ammonium perchlorate will produce = $\frac{3}{2}\times 1000=1500mol$ of molecular oxygen

Now, calculating the mass of molecular oxygen by using equation 1, we get:

Molar mass of molecular oxygen = 32 g/mol

Moles of molecular oxygen = 1500 moles

Putting values in equation 1, we get:

$1500mol=\frac{\text{Mass of molecular oxygen}}{32g/mol}\\\\\text{Mass of molecular oxygen}=(1500mol\times 32g/mol)=48000g=4.8\times 10^4g$

Hence, the mass of molecular oxygen produced is $4.8\times 10^4g$