for a combination reaction, it was calculated that 7.59g of A would exactly react with 4.88g of B. these amounts were reacted, and 9.04g of product was isolated. what was the percentage yield of reaction??
For a combination reaction, you have
A + B ==> C
A = 7.59g + B of 4.88 = 12.47 grams as the theoretical yield.
%yield = (mass product/theoretical yield)*100 = ??
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To determine the percentage yield of the reaction, you need to compare the actual yield of the product with the theoretical yield.
Step 1: Calculate the molar masses of A and B.
You can find the molar masses of elements A and B on the periodic table. Let's assume their molar masses are:
Molar mass of A = MA
Molar mass of B = MB
Step 2: Calculate the number of moles of A and B.
Use the formula:
Number of moles = Mass of substance / Molar mass
Number of moles of A = 7.59g / MA
Number of moles of B = 4.88g / MB
Step 3: Determine the limiting reactant.
The limiting reactant is the reactant that gets completely consumed during the reaction and determines the maximum amount of product that can be formed. To determine the limiting reactant, compare the number of moles of A and B using their stoichiometric coefficients in the balanced equation.
Assuming the balanced equation is: A + B -> Product
Let's say the stoichiometric coefficient of A is a and the stoichiometric coefficient of B is b.
a moles of A react with b moles of B to produce a certain amount of product.
Step 4: Calculate the theoretical yield of the product.
The theoretical yield is the maximum amount of product that can be formed based on the stoichiometry of the balanced equation.
To find the theoretical yield, use the limiting reactant (either A or B) and its stoichiometric coefficient.
Theoretical yield = (Number of moles of limiting reactant) x (Molar mass of product) / b
Step 5: Calculate the percentage yield of the reaction.
The percentage yield is the ratio of the actual yield (9.04g) to the theoretical yield, multiplied by 100.
Percentage yield = (Actual yield / Theoretical yield) x 100
Note: If the theoretical yield is unknown, you would need additional information, such as the balanced equation or the molar masses of the reactants and products, to calculate it accurately.
To determine the percentage yield of a reaction, you need to compare the actual yield (the amount of product obtained) with the theoretical yield (the maximum amount of product that should have been obtained according to stoichiometry).
In this case, the question provides the masses of reactants and the mass of the product, so we can calculate the theoretical yield and then use the formula:
Percentage Yield = (Actual Yield / Theoretical Yield) * 100
1. Start by calculating the number of moles of reactants A and B using their respective masses:
Moles of A = Mass of A / Molar mass of A
Moles of B = Mass of B / Molar mass of B
2. Next, determine the stoichiometric ratio of A to B based on the balanced chemical equation for the reaction. For example, if the reaction is:
A + B -> Product
And the balanced equation tells us that the ratio of A to B is 2:3, then:
Moles of A / 2 = Moles of B / 3
Rearrange the equation to solve for the moles of B:
Moles of B = (Moles of A * 3) / 2
3. Calculate the number of moles of product that should have been obtained based on the stoichiometry:
Moles of Product = Moles of B (or Moles of A * 3/2)
4. Convert the moles of product to grams using the molar mass of the product:
Mass of Theoretical Yield = Moles of Product * Molar mass of Product
5. Now that you have the actual yield from the question and the theoretical yield calculated above, you can calculate the percentage yield:
Percentage Yield = (Actual Yield / Theoretical Yield) * 100
Substitute the given values into the equation to find the answer.
Note: Make sure all molar masses are in grams per mole, and use the correct balanced chemical equation and stoichiometric ratios for accurate calculations.