How many moles of CO2 will be produced if 9.0 moles of O2 completely react?
is it 9.0 mol of CO2?
How many moles of CO2 will be produced if 9.0 moles of O2 completely react?
need help
Well, remember that in the reaction between O2 and CO2, the ratio is 2:2. So if 9.0 moles of O2 react completely, we'd need an equal number of moles of CO2. But since the coefficient of CO2 is 2, we'd actually need twice as many moles of CO2. So the answer is... drumroll please... 18.0 moles of CO2! It's like a two-for-one special.
To determine the number of moles of CO2 produced, we need to first balance the chemical equation for the reaction involving O2 and CO2.
The balanced chemical equation for the combustion of hydrocarbon in oxygen is:
CnHm + (n/2)O2 → nCO2 + m/2 H2O
In this case, we are only considering the reaction between O2 and CO2. So, the equation becomes:
O2 → CO2
From the balanced equation, we can see that the stoichiometry is 1:1, meaning that for every mole of O2 reacted, one mole of CO2 is produced.
Therefore, if 9.0 moles of O2 completely react, 9.0 moles of CO2 will be produced. So, your initial guess of 9.0 mol of CO2 is correct.
To determine the number of moles of CO2 produced when 9.0 moles of O2 completely react, we need to use the balanced chemical equation for the reaction in question. Since you haven't provided the specific reaction, I'll use a commonly known combustion reaction of methane as an example:
CH4 + 2O2 → CO2 + 2H2O
According to this balanced equation, one mole of methane (CH4) reacts with two moles of oxygen (O2) to produce one mole of carbon dioxide (CO2) and two moles of water (H2O).
In this case, we want to find the moles of CO2 produced when 9.0 moles of O2 react. By examining the balanced equation, we can see that the molar ratio between O2 and CO2 is 2:1. This means that for every 2 moles of O2, we will produce 1 mole of CO2.
To calculate the moles of CO2 produced, we can set up a proportion:
2 mol O2 / 1 mol CO2 = 9.0 mol O2 / x mol CO2
Simplifying this equation, we find:
x mol CO2 = (9.0 mol O2 * 1 mol CO2) / 2 mol O2
x mol CO2 = 4.5 mol CO2
Therefore, when 9.0 moles of O2 completely react, it will produce 4.5 moles of CO2. So, the answer is 4.5 mol of CO2, not 9.0 mol.
It depends on what was being combusted.
Supposing the simplest case, where carbon is being burnt:
C + O2 → CO2
(9.0 mol O2) x (1 mol CO2 / 1 mol O2) = 9.0 mol CO2
The answer would be different if the fuel contained any oxygen atoms, for example, alcohol.