need formula to this. Carbon monoxide reacts with oxygen to produce carbon dioxide. If 3.0 Liters of carbon monoxide at STP, how many liters of oxygen are required to run the reaction
2CO + O2 ==> 2CO2
You can use the shortcut in this problem in which L is used directly as if L were mols.
3L CO x (1 mol O2/2 mol CO) = 3L x 1/2 - 1.5 L O2 needed.
To calculate the amount of oxygen required to react with carbon monoxide, we need to determine the molar ratio between the two gases based on the balanced chemical equation for the reaction. The balanced equation for the reaction between carbon monoxide (CO) and oxygen (O2) to produce carbon dioxide (CO2) is:
2CO + O2 -> 2CO2
According to the balanced equation, for every 2 moles of carbon monoxide reacted, 1 mole of oxygen is required.
Given that we have 3.0 liters of carbon monoxide at STP (Standard Temperature and Pressure), we need to convert the volume of CO gas into moles.
At STP, 1 mole of any gas occupies 22.4 liters.
To convert 3.0 liters of CO to moles, we use the conversion factor:
1 mole CO = 22.4 liters CO
Thus, the number of moles of CO is:
3.0 liters CO * (1 mole CO / 22.4 liters CO) = 0.134 mole CO
Now, using the molar ratio from the balanced equation, we determine the number of moles of O2 required:
For 2 moles of CO, we need 1 mole of O2.
So, the number of moles of O2 required is:
0.134 mole CO * (1 mole O2 / 2 moles CO) = 0.067 mole O2
Finally, we convert the number of moles of O2 back to the volume of gas at STP:
0.067 mole O2 * (22.4 liters O2 / 1 mole O2) = 1.50 liters O2
Therefore, to run the reaction, 1.50 liters of oxygen are required.