For the reaction 2CH3OH + 3O2 → 2CO2+ 4H2O, what is the maximum amount of CO2 which could be formed from 13.97 g of CH3OH and 5.45 g of O2?
Consider the reaction H3PO4 + 3NaOH → Na3PO4 + 3H2O. How much Na3PO4
can be prepared by the reaction of 3.43 g of H3PO4 with an excess of NaOH?
For the reaction ?Fe+?H2O → ?Fe3O4 +?H2, what is the maximum amount of Fe3O4(231.533 g/mol) which could be formed from 12.34 mol of Fe (55.845 g/mol) and 8.74 mol of H2O (18.0153g/mol)?
These are all basically the same. For the first one,
it takes 3 moles of O2 for every 2 moles of CH3OH.
13.97g CH3OH = 0.436 moles
5.45g O2 = 0.170 moles
3/2 * 0.436 > 0.170, so the O2 limits the reaction. Each 3 moles of O2 produces 2 moles of CO2, so we will get
2/3 * 0.170 = 0.114 moles CO2
That is 5.00 g CO2
Do the others the same way.
Thanks Steve!!! :)
and steve, does the answers also come In g or what???!!!
nvm steve, thanks!!! ~.~
Steve, I still don't get it. Can you help me with the second question and the third one please??? I'm still a new learner at this kinda questions!!! :( :( :(
To find the maximum amount of CO2 that can be formed from 13.97 g of CH3OH and 5.45 g of O2, you need to use the concept of limiting reactants.
Step 1: Convert the mass of CH3OH to moles.
The molar mass of CH3OH is 32.04 g/mol.
Moles of CH3OH = (mass of CH3OH)/(molar mass of CH3OH)
Moles of CH3OH = 13.97 g / 32.04 g/mol
Step 2: Convert the mass of O2 to moles.
The molar mass of O2 is 32.00 g/mol.
Moles of O2 = (mass of O2)/(molar mass of O2)
Moles of O2 = 5.45 g / 32.00 g/mol
Step 3: Determine the limiting reactant.
Compare the mole ratio of CH3OH and O2 in the balanced chemical equation.
From the balanced equation, 2 moles of CH3OH react with 3 moles of O2 to form 2 moles of CO2.
So, the mole ratio of CH3OH to O2 is 2:3.
To determine the limiting reactant, divide the moles of CH3OH by 2, and divide the moles of O2 by 3.
Dividing moles of CH3OH by 2 gives the number of moles of O2 required if all the CH3OH were to react.
Dividing moles of O2 by 3 gives the number of moles of CH3OH required if all the O2 were to react.
Step 4: Identify the limiting reactant.
Compare the calculated number of moles of CH3OH required if all the O2 were to react and the calculated number of moles of O2 required if all the CH3OH were to react.
The reactant with the lower calculated number of moles is the limiting reactant.
Step 5: Calculate the maximum amount of CO2 that can be formed.
Using the limiting reactant, determine the amount of CO2 formed.
From the balanced equation, 2 moles of CH3OH react to form 2 moles of CO2.
So, the moles of CO2 formed is equal to the moles of the limiting reactant.
Finally, convert moles of CO2 to grams using the molar mass of CO2 to find the maximum amount of CO2 that can be formed.
Follow the same step-by-step process for the other two questions involving the reactions H3PO4 + 3NaOH → Na3PO4 + 3H2O and ?Fe+?H2O → ?Fe3O4 +?H2, using the given masses and molar masses of the substances involved.