would it be:
O.2576/0.7086=0.3635
0.3635 X 87.65= actual yield?
A 2.30-mL sample of methane gas (density 0.112 g/cm3) was completely combusted. If the percent yield of each of the combustion products is 87.65%, calculate the actual yield in grams of carbon dioxide gas.
* chemistry - DrBob222,
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
g CO2 = moles x molar mass = theoretical yield.
Then (actual g/theoretical)*100 = %yield
You know theoretical and %yield, solve for actual yield.
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.
To calculate the actual yield of carbon dioxide gas, you need to first find the theoretical yield using the given information.
1. Determine the mass of methane gas (CH4):
Given the density of methane gas (0.112 g/cm3) and the volume of the sample (2.30 mL), you can calculate the mass of methane gas:
Mass (g) = Density (g/cm3) x Volume (mL)
Mass (g) = 0.112 g/cm3 x 2.30 mL = 0.2576 g
2. Convert the mass of methane gas to moles:
To convert grams to moles, divide the mass of methane gas by its molar mass (16 g/mol):
Moles = Mass (g) / Molar mass (g/mol)
Moles = 0.2576 g / 16 g/mol = 0.0161 mol
3. Determine the moles of carbon dioxide (CO2):
Since the combustion reaction of methane produces one mole of carbon dioxide for every mole of methane, the moles of carbon dioxide should be the same as the moles of methane, which is 0.0161 mol.
4. Calculate the theoretical yield of carbon dioxide:
To find the theoretical yield of carbon dioxide gas, multiply the moles of carbon dioxide by its molar mass (44 g/mol):
Theoretical yield (g) = Moles x Molar mass
Theoretical yield (g) = 0.0161 mol x 44 g/mol = 0.7094 g
Now that you have the theoretical yield of carbon dioxide gas, you can calculate the actual yield using the given percent yield.
5. Use percent yield formula to calculate the actual yield:
The percent yield formula is:
(actual yield / theoretical yield) * 100 = percent yield
We are given that the percent yield is 87.65%, and we need to solve for the actual yield.
(Actual yield / 0.7094 g) * 100 = 87.65%
Solving for the actual yield:
Actual yield = (87.65% / 100) * 0.7094 g
Actual yield = 0.8765 * 0.7094 g
Actual yield = 0.6224 g
Therefore, the actual yield of carbon dioxide gas is 0.6224 grams.