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.
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.
would it be:
O.2576/0.7086=0.3635
0.3635 X 87.65= actual yield?
responded above.
To calculate the actual yield of carbon dioxide gas, we need to consider the density of methane gas, the volume of the sample, and the percent yield of the combustion reaction.
1. Start by calculating the mass of the methane gas sample.
Mass = Volume × Density
Mass = 2.30 mL × 0.112 g/cm3
2. Convert the mass from grams to kilograms.
Mass (kg) = Mass (g) / 1000
3. Use the balanced chemical equation for the combustion of methane to determine the molar ratio between methane and carbon dioxide. The balanced equation is:
CH4 + 2O2 → CO2 + 2H2O
4. Convert the mass of methane gas to moles using its molar mass. The molar mass of methane (CH4) is 16.04 g/mol.
Moles of methane = Mass of methane / Molar mass of methane
5. Since the mole ratio is 1:1 for methane and carbon dioxide, the moles of carbon dioxide produced will be equal to the moles of methane.
6. Multiply the moles of carbon dioxide by the molar mass of carbon dioxide (44.01 g/mol) to obtain the mass of carbon dioxide produced.
Mass of carbon dioxide = Moles of carbon dioxide × Molar mass of carbon dioxide
7. Finally, multiply the mass of carbon dioxide by the percent yield (87.65%) to obtain the actual yield.
Actual yield of carbon dioxide = Mass of carbon dioxide × Percent yield/100
Remember to perform all the necessary unit conversions and calculations to get the final answer.
Note: It's important to use accurate density values and ensure that the units are consistent throughout the calculation.