What volume (in Liters) of oxygen must react to form 17.0L of carbon dioxide according to the following balanced equation:
2CO(g) + O2(g) --> 2CO2(g)
17.0 L CO2 x (1 moles O2/2 moles CO2) = 17.0 x (1/2) = 8.5 L
did i do this problem correctly
Yes, and very good. In fact, superb.
Yes, you did the problem correctly. Your calculation is accurate.
To solve this problem, you used the coefficients from the balanced equation to determine the mole ratio between CO2 and O2. According to the equation, 2 moles of CO2 react with 1 mole of O2.
Then, you set up a conversion factor using this mole ratio: 1 mole O2/2 moles CO2.
Finally, you multiplied the given volume of CO2 (17.0 L) by this conversion factor to find the volume of O2 required:
17.0 L CO2 x (1 mole O2/2 moles CO2) = 17.0 x (1/2) = 8.5 L O2
Thus, 8.5 liters of oxygen must react to form 17.0 liters of carbon dioxide.