Respuesta :
Answer:
The percent yield of the reaction is 86.2 %
Explanation:
Step 1: Data given
Mass of CH4 = 32.0 grams
Molar mass CH4 = 16.04 g/mol
Mass of CO2 = 75.9 grams
Molar mass CO2 = 44.01 g/mol
Step 2: The balanced equation
CH4 + 2O2 → CO2 + 2H2O
Step 3: Claculate moles CH4
Moles CH4 = mass CH4 / molar mass CH4
Moles CH4 = 32.0 grams / 16.04 g/mol
Moles CH4 = 2.00 moles
Step 4: Calculate moles CO2
For 1 mol CH4 we need 2 moles O2 to produce 1 mol CO2 and 2 moles H2O
For 2.00 moles CH4 we'll have 2.00 moles CO2
Step 5: Calculate mass CO2
Mass CO2 = moles CO2 * molar mass CO2
Mass CO2 = 2.00 moles * 44.01 g/mol
Mass CO2 = 88.02 grams
Step 6: Calculate percent yield
Percent yield = (actual mass / theoretical mass) * 100 %
Percent yield = (75.9 grams / 88.02 grams) * 100%
PErcent yield = 86.2 %
The percent yield of the reaction is 86.2 %
Answer:
86.25%
Explanation:
Step 1:
The balanced equation for the reaction between CH4 and O2. This is given below:
CH4 + 2O2 —> CO2 + 2H2O
Step 2:
Determination of the mass of CH4 that reacted and the mass of CO2 produced from the balanced equation. This is shown below:
Molar Mass of CH4 = 12 + (4x1) = 12 + 4 = 16g/mol
Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol
From the balanced equation:
16g of CH4 reacted.
44g of CO2 is produced.
Step 3:
Determination of the theoretical yield of CO2. This is show below:
From the balanced equation above,
16g of CH4 produced 44g of CO2.
Therefore, 32g of CH4 will produce = (32x44)/16 = 88g of CO2.
Therefore, the theoretical yield of CO2 is 88g.
Step 4:
Determination of the percentage yield of CO2. This is shown below:
Actual yield = 75.9g
Theoretical yield = 88g
Percentage yield =?
Percentage yield = Actual yield /Theoretical yield x100
Percentage yield = 75.9/88 x 100
Percentage yield = 86.25%
Therefore, the percentage yield of CO2 is 86.25%
