Answer:
Percentage yield = 57.57%
Explanation:
Given data:
Actual yield of carbondioxide = 38.0 g
Mass of propane = 22.05 g
Percentage yield = ?
Solution:
Chemical equation:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
Number of moles of propane:
Number of moles of propane = mass / molar mass
Number of moles of propane = 22.05 g/ 44 g/mol
Number of moles of propane = 0.5 mol
Now we compare the moles of carbon dioxide with moles of propane.
C₃H₈ : CO₂
1 : 3
0.5 : 3×0.5 = 1.5 mol
Mass of carbondioxide:
Mass of carbondioxide = moles × molar mass
Mass of carbondioxide = 1.5 mol × 44 g/mol
Mass of carbondioxide = 66 g
Percentage yield:
Percentage yield = actual yield / theoretical yield × 100
Percentage yield = 38 g/ 66 g × 100
Percentage yield = 57.57%
The percentage yield of the reaction is 57.57%
Propane is an alkane whose chemical formula is [tex]C_3H_8[/tex]. It is a gas.
Given, the produced carbon dioxide is 38.0 g
Mass of propane is 22.05 g
The reaction is
[tex]\rm C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O[/tex]
Step1: Calculating the moles of propane
[tex]\rm Number\;of \;moles= \dfrac{mass}{molar\;mass}\\\\\\Number\;of \;moles\;propane=\dfrac{22.05 g}{44 g/mol} = 0.5 \;mol[/tex]
Step2: Compare the moles of Carbon dioxide to the mole of propane C₃H₈ : CO₂
1 : 3
0.5 : 3 × 0.5 = 1.5 mol
Step3: Calculating the mass of carbon dioxide
Mass of carbon dioxide = moles × molar mass
Mass of carbon dioxide = 1.5 mol × 44 g/mol = 66 g
Step4: Calculating the percentage yield
[tex]\rm Percentage\; yield = \dfrac{ actual\; yield}{theoretical\; yield} \times 100\\\\\\Percentage\; yield = \dfrac{ 38 g}{66 g} \times 100 = 57.57\%[/tex]
Thus, the percentage yield is 57.57%.
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