Question

If 88g of ${C_3}{H_8}$ and 160g of ${O_2}$ are allowed to react to form $C{O_2}$ and ${H_2}O$, how many grams of $C{O_2}$ will be formed.
A.33g
B.60g
C.132g
D.264g
E.None of the above

Answer 1

Hint: We have to calculate the moles of carbon dioxide from propane and the moles of carbon dioxide from oxygen. From the calculated moles of carbon dioxide from each reagent, we have to predict the limiting reagent. The grams of carbon dioxide formed are calculated from moles of carbon dioxide of limiting reagent and the molar mass of carbon dioxide.

Complete step by step answer:
Given data contains,
Mass of ${C_3}{H_8}$ is 88g.
Mass of ${O_2}$ is 160g.
We obtain the products carbon dioxide and water from the combustion reaction of propane. We can write the balanced chemical equation as,
${C_3}{H_8} + 5{O_2} \to 3C{O_2} + 4{H_2}O$
We know the molar mass of ${C_3}{H_8}$ is 44.1g/mol.
We know the molar mass of ${O_2}$ is 32g/mol.
We know the molar mass of $C{O_2}$ is 44g/mol.
Let us now calculate the moles of carbon dioxide from propane.
Moles of carbon dioxide = $\left( {88g \times \dfrac{{1mol}}{{44g}}} \right) \times \left( {\dfrac{{3molCO{ _2}}}{{1mol{C_3}{H_8}}}} \right)$
Moles of carbon dioxide = $6moles$
The moles of carbon dioxide obtained from propane are six moles.
Let us now calculate the moles of carbon dioxide from oxygen.
Moles of carbon dioxide=$\left( {160g \times \dfrac{{1mol{O_2}}}{{32g}}} \right) \times \left( {\dfrac{{3molCO{ _2}}}{{5mol{O_2}}}} \right)$
Moles of carbon dioxide = $3moles$
The moles of carbon dioxide obtained from oxygen are three moles.
From the calculated moles of carbon dioxide from oxygen and calculated moles of carbon dioxide from propane, we can see that oxygen is the limiting reagent.
So, we have to now calculate the grams of carbon dioxide from moles of carbon dioxide formed from oxygen and the molar mass of oxygen.
Grams of carbon dioxide = $3\;moles\;C{O_2} \times \dfrac{{44g\;C{O_2}}\;}{{1\;mol\;C{O_2}}}$
Grams of carbon dioxide = $132gC{O_2}$
The grams of carbon dioxide is $132g$.

Therefore, the option (C) is correct.

Note:
As we know that the burning of fossil fuels by humans is the largest source of releases of carbon dioxide that is one of the greenhouse gases that permits radiative forcing and contributes to global warming. A small part of hydrocarbon-based fuels are biofuels obtained from atmospheric carbon dioxide, and therefore do not rise the net amount of carbon dioxide in the atmosphere. Combustion of fossil fuels produces sulfuric and nitric acids that fall to Earth as acid rain, affecting both natural areas and the built environment.