2CO + O2 ==> 2CO2
When all gases and at the same T and P, one may use a shortcut in which volumes may be used as if they were mols.
0.677 L CO + (2 mols O2/1 mol CO) = L O2 gas needed.
Assume all volume measurements are made
at the same temperature and pressure.
Thanks in advance for all help!!
When all gases and at the same T and P, one may use a shortcut in which volumes may be used as if they were mols.
0.677 L CO + (2 mols O2/1 mol CO) = L O2 gas needed.
mols CO = 0.677 L x (1 mol/22.4L) = 0.0302.
Now use the coefficients in the balanced equation to convert mols CO to mols O2. That's 0.0302 mols CO x (1 mol O2/2 mols CO) = 0.0302 x 1/2 = 0.0151 mols O2 needed to completely burn the CO.
Now convert mols O2 to L.
0.0151 mols O2 x (22.4 L/mol) = 0.338 L.
Back to the shortcut way. You see I converted to mols by dividing by 22.4 in the first step and converted back to L by multiplying by 22.4 L in the last step. So the shortcut method just doesn't divide by 22.4 first because we know it will cancel in the last step anyway. So the shortcut way we simply convert L CO to L O2 by using the coefficients in the balanced equation.
By the way, we can convert any mol quantity in an equation to any other mol quantity in the same equation by using the coefficients in the balanced equation.
0.677 L CO x (1 mol O2/2 mols CO) = 0.677 x 1/2 = 0.338 L.
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The balanced chemical equation for the reaction between carbon monoxide gas (CO) and oxygen gas (O2) to form carbon dioxide gas (CO2) is:
2CO + O2 -> 2CO2
From the balanced equation, you can see that 2 moles of carbon monoxide react with 1 mole of oxygen to form 2 moles of carbon dioxide.
First, convert the given volume of carbon monoxide gas (0.677 L) into moles using the Ideal Gas Law equation:
PV = nRT
Assuming temperature and pressure are constant, and using the molar volume (22.4 L/mol) at standard temperature and pressure (STP), you can calculate the number of moles:
n = V/22.4
n = 0.677 L / 22.4 L/mol
Next, use the stoichiometry of the balanced equation to find the number of moles of oxygen needed:
1 mole of CO reacts with 1/2 mole of O2
Therefore, the number of moles of oxygen gas needed is:
n(O2) = (1/2) * n(CO)
Finally, convert the moles of oxygen gas back into volume using the molar volume at STP:
V(O2) = n(O2) * 22.4 L/mol
Plug in the value of n(O2) calculated in the previous step to find the volume of oxygen gas needed to react completely with carbon monoxide gas.