Calculation of Percentage Yield

To calculate the percentage yield, we need to compare the actual yield (the amount of oxygen produced) with the theoretical yield (the amount of oxygen that should have been produced based on stoichiometry).

Stoichiometry of the Reaction

The balanced chemical equation for the decomposition of KCLO3 is:

2 KCLO3 -> 2 KCl + 3 O2

From the balanced equation, we can see that 2 moles of KCLO3 produce 3 moles of O2.

Calculating the Theoretical Yield

To calculate the theoretical yield of oxygen, we need to convert the given mass of KCLO3 to moles and then use the stoichiometric ratio to find the corresponding moles of O2.

The molar mass of KCLO3 is:
K: 39.10 g/mol
Cl: 35.45 g/mol
O: 16.00 g/mol

Molar mass of KCLO3 = 39.10 + 35.45 + (3 * 16.00) = 122.55 g/mol

Given mass of KCLO3 = 61.25 g

Number of moles of KCLO3 = mass / molar mass = 61.25 g / 122.55 g/mol = 0.500 mol

Using the stoichiometric ratio, we can calculate the moles of O2 produced:

Moles of O2 = (3/2) * moles of KCLO3 = (3/2) * 0.500 mol = 0.750 mol

The molar mass of O2 is 32.00 g/mol. Therefore, the theoretical yield of oxygen is:

Theoretical yield of O2 = moles of O2 * molar mass = 0.750 mol * 32.00 g/mol = 24.00 g

Calculating the Percentage Yield

The percentage yield is calculated by dividing the actual yield by the theoretical yield and multiplying by 100.

Given actual yield of O2 = 18 g

Percentage yield = (actual yield / theoretical yield) * 100
= (18 g / 24.00 g) * 100
= 75%

Explanation

The percentage yield is a measure of the efficiency of a chemical reaction. It represents the ratio of the actual amount of product obtained to the maximum amount that could have been obtained based on stoichiometry.

In this case, the given mass of KCLO3 is converted to moles, and then using the stoichiometric ratio, the corresponding moles of O2 are calculated. The molar mass of O2 is used to convert the moles to grams, giving the theoretical yield of oxygen.

The actual yield of oxygen is given as 18 g. To calculate the percentage yield, the actual yield is divided by the theoretical yield and multiplied by 100.

The percentage yield of 75% indicates that 75% of the maximum possible amount of oxygen was obtained in the reaction. The remaining 25% may be lost due to various factors such as incomplete reaction, side reactions, or experimental errors.

It is important to note that the percentage yield can never be greater than 100%. A percentage yield of 100% would indicate a perfect reaction where all reactants were converted to products without

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