Question

What mass of oxygen forms from 71.89 g CO2?

Use the periodic table to find molar masses.
71.89 g CO2 =
gO₂
rom
DONE
2.18

Answer 1

`\large \boxed{\text{52.27 g}}`

Step-by-step explanation:

1. Molar masses

(a) CO₂

1 C = 1 × 12.01 u = 12.01 u

2 O = 2 × 16.00 u = 32.00 u

TOTAL = 44.01 u

(b) O₂

2 O = 2 × 16.00 u = 32.00 u

2. Mass of oxygen produced

We will need a chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ: 44.01 32.00

CO₂ ⟶ C + O₂

m/g: 71.89

So, 32.00 g of oxygen form from 44.01 g of CO₂

`\text{Mass of O}_(2) = \text{71.89 g CO}_(2) * \frac{\text{32.00 g O}_(2)}{\text{44.01 g CO}_(2)} = \textbf{52.27 g O}_(2)\\\\\text{The mass of O$_(2)$ produced is $\large \boxed{\textbf{52.27 g}}$}`