Question

If you need to produce 66 grams of carbon dioxide. How many liters of oxygen gas do you need?

Answer 1

The question requires us to calculate the amount, in liters, of oxygen gas (O2) needed to produce 66g of carbon dioxide (CO2).

To produce CO2, we can combine carbon monoxide (CO) and oxygen gas (O2) as in the following reaction:

`2CO_((g))+O_(2(g))\rightarrow2CO_(2(g))`

Now that we have the reaction and its stoichiometric coefficients, we can stabilish a stoichiometric relation between O2 and CO2:

1 mol O2 -------------- 2 mol CO2

Then, we need to calculate how many moles of CO2 are in 66g of this compound.

Knowing that the molar mass of CO2 is 44 g/mol (molar mass = (1 * 12) + (2 * 16) = 44 g/mol), we can calculate:

44g CO2 ---------- 1 mol

66g CO2 ---------- x

Solving for x, we have that there are 1.5 moles of CO2 in 66g of this gas.

Now, we use the stoichiometric relation estabilished before to calculate how much O2 is necessary to produce 1.5 moles of CO2:

1 mol O2 -------------- 2 mol CO2

y ------------- 1.5 mol CO2

Solving for y, we have that 0.75 moles of O2 are necessary to obtain 1.5 moles (or 66g) of CO2.

Since the question asks the volume, in liters, of O2, we calculate the volume of this gas considering the Standard Temperature and Pressure conditions (STP), where 1 mol of a gas corresponds to 22.4 L of the same gas:

1 mol O2 ---------- 22.4 L O2

0.75 mol O2 ---- z

Now, solving for z, we have that 16.8 L of O2 are necessary to obtain 66g of CO2.