Balance the equation below. How many moles of CO2 are produced when 40.0 grams o

Question

Balance the equation below.
How many moles of CO2 are produced when 40.0 grams of C6H12O6 react in this equation?
How many grams of CO2 are produced?
If only 13.2 grams of CO2 are produced what is the percent yield of CO2?
How many grams of C6H12O6 would be needed to form 7.50g of C2H5OH?
___ C6H12O6->____C2H5OH+____CO2

Explanation / Answer

The balanced equation is C6H12O6 -> 2C2H5OH + 2CO2 by stoichoimetry clearly 1 mol c6h12o6 gives 2 mol co2 mol. wt of c6h12o6 = 180 mol of c6h12o6 = 0.222 mol co2 evolved = 2*0.222 = 0.444 mol wt of co2 = 44 gms of co2 produced = 19.56gm. by complete consumption of c6h12o6 19.56gm co2 must be produced but given only 13.2 gm is formed hence % yield = (13.2/19.56)*100 = 67.5% mol wt of c2h5oh = 46gm so moles of c2h5oh reqd = 7.5/46 = 0.163mol by stoichoimetry, mol of c6h12o6 needed = 0.5*0.163 = 0.0815 hence amt of c6h12o6 needed = 14.674gm

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