Question

2 gm iron pyrite is burnt with O2 to form Fe2O3 and SO2 .the mass of SO2 produced is​

Answer 1

Answer:

2gm

Explanation:

we can say that easily because it is like that only

Answer 2

The mass of sulfur dioxide produced is 2.125 grams

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 $FeS_2$ = 2 g

Molar mass of $FeS_2$ = 120 g/mol

Putting values in equation 1, we get:

$\text{Moles of }FeS_2=\frac{2g}{120g/mol}=0.0166mol$

The chemical equation for the reaction of $FeS_2$ and oxygen gas follows:

$4FeS_2+11O_2\rightarrow 2Fe_2O_3+8SO_2$

By Stoichiometry of the reaction:

4 moles of $FeS_2$ produces 8 moles of sulfur dioxide

So, 0.0166 moles of $FeS_2$ will produce = $\frac{8}[4}\times 0.0166=0.0332mol$ of sulfur dioxide

Now, calculating the mass of sulfur dioxide from equation 1, we get:

Molar mass of sulfur dioxide = 64 g/mol

Moles of sulfur dioxide = 0.0332 moles

Putting values in equation 1, we get:

$0.0332mol=\frac{\text{Mass of sulfur dioxide}}{64g/mol}\\\\\text{Mass of sulfur dioxide}=(0.0332mol\times 64g/mol)=2.125g$

Learn more about number of moles and stoichiometry:

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