Posted by gary on Saturday, October 23, 2010 at 5:16pm.
No. Are you trying to say that you start with 0.2576g CH4 and you end up with 0.3635 x 87.65 = 31.86 g CO2? The theoretical yield is ONLY 0.708 grams; how can the actual yield exceed that by 44 times.
CH4 + 2O2 ==> CO2 + 2H2O
g CH4 = 2.30 mL x 0.112 g/mL = 0.2576
moles CH4 = 0.2576/16 = 0.0161
moles CO2 must be 0.0161 also from the coefficients in the balanced equation.
g CO2 = moles x molar mass = theoretical yield.
0.0161 moles CO2 x (44 g CO2/mole CO2) = 0.708 g CO2. This is the theoretical yield.
Then (actual g/theoretical)*100 = %yield
You know theoretical and %yield, solve for actual yield.
(actual yield/theor yield)*100 = 87.65%
(actual yield/0.708 g)*100 = 87.65%
(actual yield/0.708) = 0.8765
(actual yield) = 0.8765*0.708 = 0.6209 which rounds to 0.621 to three s.f.
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