what mass of oxygen forms from 71.89 g co₂? use the periodic table to find molar masses. 71.89 g co₂ = g o₂…

Explanation:

Step1: Calculate molar mass of CO₂

The molar mass of C is 12.01 g/mol and O is 16.00 g/mol. For CO₂, $M_{CO_2}=12.01 + 2\times16.00=44.01$ g/mol.

Step2: Calculate moles of CO₂

$n_{CO_2}=\frac{m_{CO_2}}{M_{CO_2}}=\frac{71.89}{44.01}\approx1.6335$ mol.

Step3: Determine mole - ratio between CO₂ and O₂

In CO₂, there are 2 moles of O for every 1 mole of CO₂. When CO₂ decomposes to form O₂, the mole - ratio of CO₂ to O₂ is 1:1 (since all the oxygen in CO₂ can potentially form O₂). So, $n_{O_2}=n_{CO_2}\times1 = 1.6335$ mol.

Step4: Calculate mass of O₂

The molar mass of O₂ is $M_{O_2}=2\times16.00 = 32.00$ g/mol. Then $m_{O_2}=n_{O_2}\times M_{O_2}=1.6335\times32.00 = 52.272$ g.

Answer:

52.27 g (rounded to two decimal places)