125 mL of 1.00 M HCl with 9.00 g of KOH. if the yield of KCL is 7.51 g what is the percent yield of the reaction
HCl + KOH -> KCl + H2O
The procedure in this example will work the problem for you.
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To find the percent yield of a reaction, you need to know the actual yield and the theoretical yield. The actual yield is the amount of product obtained from the reaction, which in this case is given as 7.51 grams of KCl. The theoretical yield, on the other hand, is the maximum amount of product that could be obtained according to the balanced equation.
To calculate the theoretical yield of KCl, you need to determine the limiting reagent. The limiting reagent is the reactant that is completely consumed in the reaction and determines the maximum amount of product that can be formed. To find the limiting reagent, you can use the concept of stoichiometry and compare the number of moles of each reactant to the balanced equation.
Let's start by determining the number of moles of HCl and KOH:
- 125 mL of 1.00 M HCl means there are 0.125 L (or 0.125 moles) of HCl.
- 9.00 g of KOH can be converted to moles using its molar mass: (9.00 g) / (56.11 g/mol) = 0.160 moles of KOH.
Now, let's compare the number of moles of HCl and KOH to determine the limiting reagent:
From the balanced equation, the stoichiometry tells us that 1 mole of HCl reacts with 1 mole of KOH to form 1 mole of KCl.
- The moles ratio between HCl and KOH is 0.125/1 = 0.125.
- The moles ratio between KOH and KCl is 0.160/1 = 0.160.
Comparing the ratios, we can see that the ratio between HCl and KOH is smaller, which means HCl is the limiting reagent.
Since HCl is the limiting reagent, we can use its moles to calculate the theoretical yield of KCl:
The moles ratio between HCl and KCl is 1/1, which means 0.125 moles of HCl will also produce 0.125 moles of KCl.
The molar mass of KCl is 74.55 g/mol, so the theoretical yield of KCl is:
0.125 moles * 74.55 g/mol = 9.32 g of KCl.
Now that we have the actual yield (7.51 g) and the theoretical yield (9.32 g), we can calculate the percent yield:
Percent Yield = (Actual Yield / Theoretical Yield) * 100
= (7.51 g / 9.32 g) * 100
≈ 80.52%
Therefore, the percent yield of the reaction is approximately 80.52%.