The fermentation of glucose (C₆H₁₂O₆) produces ethyl alcohol (C₂H₅OH) and CO₂: C₆H₁₂O₆ → 2C₂H₅OH + 2CO₂?
a) How many moles of CO₂ are produced when 0.400 mol of C₆H₁₂O₆ reacts in this fashion?
b) How many grams of C₆H₁₂O₆ are needed to form 7.50 g of C₂H₅OH?
c) How many grams of CO₂ form when 7.50 g of C₂H₅OH are produced?
HELP ME!!!!!!!!! please.
More Questions From This User See All
Answers & Comments
Verified answer
Write a balanced equation:
C6H12O6 = 2 C2H5OH + 2 CO2
1mol C6H12O6 produced 2mol CO2
Therefore 0.400mol C6H12O6 will produce 0.800mol CO2 =Q1
1mol C6H12O6 produces 2mol C2H5OH
Molar mass C2H2OH = 46.07 g mol−1
7.5g = 7.5/46.07 = 0.1628mol
You require 0.1628/2 = 0.0814molC6H12O6
Molar mass C6H12O6 =180.16 g/mol
0.0814mol = 180.16*0.0814 = 14.66g C6H12O6 required =Q2
Molar mass CO2 = 44.010 g/mol
CO2 is produced in the same mol ratio as C2H5OH
If 7.5g C2H5OH is produced,
7.5*46.07*44.01 = 7.16g CO2 produced =Q3
You can check this:
14.66g C6H12O6 will produce7.5g C2H5OH and 7.16g CO2 = 14.66g
So it balances out exactly: the mass of the products equals the mass of the reactants.
im not gonna do it for you cuz its kind of a pain but ill explain it
A) Find the Molar Mass of C6H12O6
do this by looking at a periodic table, carbon is 12g/mol and you have 6 so 6*12 = 72 hydrogen is 1 and you have 12 so 1 * 12 = 12 etc
all them all up and you have the molar mass.. write it down and call it w
take the molar mass of CO2 and multiply by 2 because you get 2 out
save that number, ill call it x
then multiply the molar mass of C6H12O6 by .400. that will tell you how much C6H12O6 you are putting in. save that number ill call it z
x/w tells you how much 2CO2 is made from 1(C6H12O6)
take that and multiply it by z and there is your anwer in grams. Divide that by the molar mass of CO2 and thats how many moles you have
B) same thing
C) Same thing just reversed around
if you want me to solve it email me or something