How many moles of H2O are produced when 6 moles of o2 is consumed in burning meyhyl Alchohol
To determine the number of moles of H2O produced when 6 moles of O2 is consumed in burning methyl alcohol, we need to balance the chemical equation and then use stoichiometry.
First, let's write the balanced equation for the combustion of methyl alcohol (CH3OH):
2 CH3OH + 3 O2 -> 2 CO2 + 4 H2O
From the balanced equation, we can see that for every 2 moles of CH3OH, 4 moles of H2O are produced. So, the stoichiometric ratio is 2 moles of H2O for every 2 moles of CH3OH.
Now, we have 6 moles of O2, but we need to find how many moles of CH3OH are necessary to consume that amount of O2. Since the stoichiometric ratio of O2 to CH3OH is 3:2, we can set up a proportion:
3 moles of O2 / 2 moles of CH3OH = 6 moles of O2 / x moles of CH3OH
Cross multiplying, we have:
3x = 12
x = 12 / 3
x = 4
So, to consume 6 moles of O2, we need 4 moles of CH3OH.
Now, we can use the stoichiometric ratio between CH3OH and H2O to find the moles of H2O produced:
4 moles of CH3OH * (4 moles of H2O / 2 moles of CH3OH) = 8 moles of H2O
Therefore, when 6 moles of O2 is consumed in burning methyl alcohol, 8 moles of H2O are produced.