Question

What mass of oxygen forms from 71.89 g CO2?
Use the periodic table to find molar masses.
71.89 g CO2 =
go2

Answer 1

Answer:

52.28g

Explanation:

Given:

Mass of CO₂ = 71.89g

Solution:

The equation of the reaction:

                  CO₂ → C + O₂

We want to determine the mass of O₂ that will form from this reaction.

To do this, find the number of moles of CO₂:

   Number of moles of CO₂ = $\frac{mass}{molar mass}$

Molar mass of CO₂ = 12+ 2(16) = 44g/mol

   Number of moles of CO₂ = $\frac{71.89}{44}$ = 1.63mole

From the equation of the reaction:

      1mole of CO₂ will produce 1 mole of O₂

 So 1.63 mole of CO₂ also produces 1.63mole of O₂

The mass of O₂:

    Mass of O₂ = number of moles of O₂ x molar mass of O₂

Molar mass of O₂ = 2 x 16 = 32g/mol

    Mass of O₂ = 1.63 x 32 = 52.28g

Answer 2

Answer:  52.27

Explanation: you don't round