The reaction between 32.0g of CH4 and excess oxygen gas produces 75.9 of CO2 gas and some water. Determine the percent yield? Plss help :((
To calculate the percent yield of a reaction, you need to compare the actual yield (the experimental amount of the desired product) to the theoretical yield (the calculated amount of the product based on stoichiometry).
In this case, the reaction is:
CH4 + 2O2 -> CO2 + 2H2O
Given:
Mass of CH4 = 32.0 g
Mass of CO2 produced = 75.9 g
To calculate the theoretical yield of CO2, you can use the molar mass of CH4 and the stoichiometry of the balanced equation.
1. Calculate the number of moles of CH4:
moles of CH4 = mass / molar mass = 32.0 g / 16.04 g/mol = 1.993 mol
2. Calculate the number of moles of CO2 produced using the stoichiometry of the balanced equation:
From the balanced equation, you can see that 1 mole of CH4 produces 1 mole of CO2.
Therefore, moles of CO2 produced = 1.993 mol
3. Calculate the mass of CO2 based on the moles:
mass of CO2 = moles of CO2 * molar mass = 1.993 mol * 44.01 g/mol = 87.55 g
Now, you can calculate the percent yield:
Percent yield = (actual yield / theoretical yield) * 100%
Actual yield = mass of CO2 produced = 75.9 g
Theoretical yield = mass of CO2 calculated = 87.55 g
Percent yield = (75.9 g / 87.55 g) * 100% ≈ 86.8%
Therefore, the percent yield of the reaction is approximately 86.8%.
To determine the percent yield of a reaction, you need to compare the actual yield of the desired product with the theoretical yield. Theoretical yield refers to the amount of product that would be obtained if the reaction proceeded perfectly, without any losses or side reactions.
To calculate the theoretical yield, you need to use stoichiometry, which is the balanced equation of the reaction. In this case, the balanced equation is:
CH4 + 2O2 -> CO2 + 2H2O
According to the equation, one mole of methane (CH4) reacts with two moles of oxygen gas (O2) to produce one mole of carbon dioxide (CO2) and two moles of water (H2O).
First, calculate the number of moles of CH4 used in the reaction:
32.0 g CH4 x (1 mole CH4 / 16.04 g CH4) = 2.00 moles CH4
Since the reaction is said to have an excess of oxygen gas, the methane is the limiting reactant. Therefore, the number of moles of CO2 produced will be equal to the number of moles of CH4 used in the reaction.
Now, calculate the number of grams of CO2 produced:
2.00 moles CO2 x (44.01 g CO2 / 1 mole CO2) = 88.02 g CO2
The theoretical yield of CO2 is 88.02 grams.
Next, calculate the percent yield using the actual yield and the theoretical yield:
Percent Yield = (Actual Yield / Theoretical Yield) x 100
In this case, the actual yield of CO2 produced is given as 75.9 grams.
Percent Yield = (75.9 g CO2 / 88.02 g CO2) x 100 = 86.3%
Therefore, the percent yield of the reaction is 86.3%.