what mass of oxygen forms from 71.89 g co₂? use the periodic table to find molar masses. 71.89 g co₂ = g o₂
what mass of oxygen forms from 71.89 g co₂? use the periodic table to find molar masses. 71.89 g co₂ = g o₂
Answer
Explanation:
Step1: Calculate molar mass of $CO_2$
The molar mass of $C$ is $12.01\ g/mol$ and of $O$ is $16.00\ g/mol$. So molar mass of $CO_2$ is $12.01 + 2\times16.00=44.01\ g/mol$.
Step2: Calculate moles of $CO_2$
Moles of $CO_2=\frac{mass}{molar\ mass}=\frac{71.89\ g}{44.01\ g/mol}\approx1.6335\ mol$.
Step3: Determine mole - ratio of $CO_2$ to $O_2$
From the chemical equation (e.g., $CO_2$ decomposition or relevant reaction), the mole - ratio of $CO_2$ to $O_2$ is $1:1$ (assuming complete oxygen release from $CO_2$). So moles of $O_2 = 1.6335\ mol$.
Step4: Calculate mass of $O_2$
The molar mass of $O_2$ is $2\times16.00 = 32.00\ g/mol$. Mass of $O_2=moles\times molar\ mass=1.6335\ mol\times32.00\ g/mol = 52.272\ g$.
Answer:
$52.27$ (rounded to two decimal places)