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In this question, we have the following reaction, which is the cellular respiration reaction:
C6H12O6 + 6 O2 --> 6 CO2 + 6 H2O
We have:
120 grams of CO2 being produced
The molar ratio between CO2 and O2 is 6:6, which means the same amount of moles produced of CO2 will be the same amount used of O2
Now we find the number of moles of CO2, using its molar mass = 44.01g/mol
44.01 grams = 1 mol
120 grams = x moles
44.01x = 120
x = 120/44.01
x = 2.73 moles of CO2
If we have 2.73 moles of CO2, we will also have 2.73 moles of O2, and to find its mass, we will also use the molar mass of O2 = 32g/mol
32 grams = 1 mol
x grams = 2.73 moles
x = 2.73 * 32
x = 87.4 grams of O2
The amount required of oxygen gas to produce 120 grams of CO2 based on the cellular respiration reaction will be 87.4 grams