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)
is this correct
C G02
2
I have no idea what C GO2 over 2 is.
17.0L CO2 x (1 mole O2/2 moles CO2) = 8.5 L CO2
To determine the volume of oxygen required to form 17.0L of carbon dioxide, we need to use the balanced equation provided:
2CO(g) + O2(g) → 2CO2(g)
From the equation, we can see that for every 1 mole of O2, 2 moles of CO2 are formed. Therefore, we need to determine the number of moles of CO2 first.
To calculate the number of moles of CO2, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (we can assume it is constant)
V = volume of CO2 = 17.0L
n = number of moles
R = ideal gas constant
T = temperature (we can assume it is constant)
Since we only need the number of moles, the ideal gas law equation can be rearranged as:
n = PV/RT
Next, we need to convert the moles of CO2 to moles of O2 using the stoichiometry of the balanced equation. From the balanced equation, we can see that the ratio of O2 to CO2 is 1:2. Therefore, for every 2 moles of CO2, 1 mole of O2 is required.
Finally, we can use the moles of O2 to calculate the volume of O2 using the ideal gas law equation rearranged for volume:
V = (nRT) / P
Substituting the calculated moles from the previous step, we can find the volume of O2 required to form 17.0L of CO2.