Final answer:
To produce 5.8 grams of CO2, approximately 4.22 grams of oxygen gas is required, based on the balanced equation for the combustion of carbon, where one mole of CO2 is produced from one mole of O2.
Step-by-step explanation:
To determine the mass of oxygen gas (O2) required to produce 5.8 grams of CO2, we need to use the balanced chemical equation for the combustion of carbon (or a carbon-containing compound) which is often represented as C + O2 → CO2. However, the student has not provided the complete reaction which includes the reactants involved, so we will assume the use of pure carbon in its simplest form:
C + O2 → CO2
To find the mass of oxygen needed, we can start by finding the moles of CO2 produced from the mass given:
(5.8 grams CO2) × (1 mole CO2 / 44.01 g CO2) = 0.1318 moles CO2
From the equation, one mole of CO2 is produced from one mole of O2, so 0.1318 moles of CO2 would require 0.1318 moles of O2:
0.1318 moles O2 × (32.00 g O2 / 1 mole O2) = 4.2176 grams O2
Therefore, approximately 4.22 grams of O2 is required to produce 5.8 grams of CO2.