Calculations based on chemical equations help please !!?
how many moles of CO2 are produced when 0.400 mol of C6H12O6 reacts in this fashion?
how many grams of C6H12O6 are needed to form 7.50g of C2H5OH?
how many grams of CO2 form when 7.50 g of C2H5OH are produced?
Answer:
The balanced equation is
C6H12O6 >> 2 C2H5OH + 2 CO2
the ratio between C6H12O6 and CO2 is 1 : 2
1 : 2 = 0.400 : x
x = 0.800 moles
Molar mass C2H5OH = 46 g / mol
7.50 g / 46 = 0.163 moles
the ratio between C6H12O6 and C2H5OH is 1 : 2
1 : 2 = x : 0.163
x = 0.0815 moles of C6H12O6 needed
molar mass C6H12O6 = 180 g/mol
180 x 0.0815 = 14.7 g
the ratio between C2H5OH and CO2 is 2 : 2 so will be produced 0.163 moles of CO2
molar mass = 44 g/mol
44 x 0.163 = 7.17 g
I think you mis-typed the first product, leaving off an OH at the end... With that there, read on.
To get values from the equation, you need to take the stoichiometry into consideration. Just turn it into ratios and it will make the math much easier.
ratio is 1:2:2
so .4mol of the 1 reactant means .8mol of each product
For the next two you need to convert the grams into molecular weights first.
C2H5OH = 46g/mol (appox)
7.5g = .163mol
C6H12O6 = 180g/mol (appox)
you need half the reactant for each product, so half of .163mol is .0815mol. and .0815mol equals 14.67 grams of C6H12O6.
Since the ratio is the same for the last product, you can calculate the molecular weight, 44g/mol (approx) and apply it to the same number of moles as C2H5OH, .163. Which comes out to be 7.172g.
C6H12O6 ----> 2 C2H5OH + 2 CO2
The equation shows you that 1 mole of C6H12O6 reacts to produce 2 moles of CO2, so 0.8 moles of CO2 are produced from 0.4 moles of C6H12O6.
7.5g of C2H5OH is 7.5/46.07 moles (0.1628 moles) so you will need 0.0814 moles of C6H12O6 which is 0.0814x180.1= 14.66 grams.
0.1628 moles of C2H5OH produced so you will get 0.1628 moles of CO2 or 0.1628x44.011=7.165 grams CO2.
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