Calculate % yield of reaction if 1 kg potassium bicarbonate produces 110gram of carbon dioxide upon strong heating?

Question

Answer

Calculation of % Yield of Reaction

Given:

Mass of potassium bicarbonate = 1 kg

Mass of carbon dioxide produced = 110 g

Step 1: Calculate the theoretical yield of the reaction

The balanced chemical equation for the reaction is:

2KHCO₃ → K₂CO₃ + CO₂ + H₂O

The molar mass of KHCO₃ is 100.11 g/mol

Number of moles of KHCO₃ = (1000 g) / (100.11 g/mol) = 9.994 mol

According to the balanced equation, 2 moles of KHCO₃ produces 1 mole of CO₂.

Number of moles of CO₂ produced = (9.994 mol / 2) = 4.997 mol

Theoretical yield of CO₂ = (4.997 mol) x (44.01 g/mol) = 220.08 g

Step 2: Calculate the % yield of the reaction

The actual yield of CO₂ produced is given as 110 g.

Percent yield = (actual yield / theoretical yield) x 100

Percent yield = (110 g / 220.08 g) x 100 = 50%

Explanation:

The percent yield of a reaction is a measure of the efficiency of the reaction. It is the ratio of the actual yield to the theoretical yield, expressed as a percentage. In this case, only 110 g of CO₂ was produced instead of the expected 220.08 g, resulting in a percent yield of 50%. There could be various reasons for the low yield, such as incomplete reactant conversion, side reactions, or loss of product during handling. Identifying and minimizing these factors is crucial for achieving better yields in chemical reactions.

Answer

According to Avogadro's law, 1 mole of every substance weighs equal to the molecular mass and contains avogadro's number of particles

According to stoichiometry:

2 moles of khco3 produce 1 mole of produce of co2

Thus 1000 g of should produce of

Thus theoretical yield of is 220 g.

But Experimental yield is 110 g.

use the formula and solve

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