For combustion of 10 grams of C4H10 excess of O2, You are obtained 25 grams of CO2
according to the reaction (to balance):
C4H10+ O2→ CO2+ H2O
Calculate the reaction yield of the reaction.
please,could anyone help me to solve this problem.
so, do you know what reaction yield means?
reaction yield=(actual yield÷theoretical yield)*100%
To calculate the reaction yield, we need to determine the limiting reactant and then use the stoichiometric ratio from the balanced equation to calculate the expected amount of CO2 that should have been produced. Then we can compare it to the actual amount obtained and calculate the yield.
Step 1: Calculate the molar mass of C4H10 (butane):
C4H10 = (4 * 12.01 g/mol) + (10 * 1.01 g/mol) = 58.12 g/mol
Step 2: Calculate the number of moles of C4H10 used:
Moles of C4H10 = Mass of C4H10 / Molar mass of C4H10
= 10 g / 58.12 g/mol
= 0.172 mol
Step 3: Use the balanced equation to determine the stoichiometric ratio between C4H10 and CO2.
From the balanced equation: 1 mol C4H10 produces 4 mol CO2.
Step 4: Calculate the expected moles of CO2 produced:
Expected moles of CO2 = Moles of C4H10 * (Moles of CO2 / Moles of C4H10 ratio)
= 0.172 mol * (4 mol CO2 / 1 mol C4H10)
= 0.688 mol
Step 5: Calculate the expected mass of CO2 produced:
Expected mass of CO2 = Expected moles of CO2 * Molar mass of CO2
= 0.688 mol * 44.01 g/mol
= 30.31 g
Step 6: Calculate the reaction yield:
Reaction yield = (Actual mass of CO2 obtained / Expected mass of CO2) * 100
= (25 g / 30.31 g) * 100
= 82.49%
Therefore, the yield of the reaction is approximately 82.49%.