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Chapter 3: Problem 72

(a) Define the terms theoretical yield, actual yield, and percent yield. (b) Why is the actual yield in a reaction almost always less than the theoretical yield? (c) Can a reaction ever have \(110 \%\) actual yield?

Short Answer

Expert verified
Theoretical yield is the maximum amount of product that can be formed from a given amount of reactants, assuming 100% efficiency. Actual yield is the amount of product obtained experimentally, which is usually less than the theoretical yield due to factors like side reactions, incomplete reactions, and product losses. Percent yield is the ratio of actual yield to theoretical yield, expressed as a percentage. Actual yield is typically less than theoretical yield because of these factors affecting reaction efficiency, and a reaction cannot have an actual yield greater than 100%, as it would imply more product is being produced than theoretically possible. An actual yield greater than 100% is typically due to experimental errors or inaccuracies in measurements.

Step by step solution

01

Definition of Theoretical Yield

Theoretical yield refers to the maximum amount of product that can be formed from a given amount of reactants in a chemical reaction. It is based on the balanced chemical equation and assumes that the reaction goes to completion with 100% efficiency.
02

Definition of Actual Yield

Actual yield is the amount of product that is actually obtained from a reaction in the laboratory or industry after accounting for side reactions, incomplete reactions, and other losses. It is typically measured experimentally and is almost always less than the theoretical yield due to various factors affecting the efficiency of the reaction.
03

Definition of Percent Yield

Percent yield is the ratio of the actual yield to the theoretical yield, expressed as a percentage. It is a measure of the efficiency of a reaction and is calculated using the following formula: \[ Percent \ Yield = \frac{Actual \ Yield}{Theoretical \ Yield} \times 100\%\]
04

Reasons for Actual Yield being less than Theoretical Yield

The actual yield is almost always less than the theoretical yield due to several factors, such as: 1. Side reactions: Sometimes, reactants may undergo other reactions besides the desired reaction, leading to formation of other products which decrease the yield of the desired product. 2. Incomplete reactions: Some reactions may not proceed to completion and the reactants are not fully consumed. This can be due to factors like equilibrium, temperature, or other conditions affecting the reaction. 3. Loss of product during purification or handling: The product may be lost during the process of separating it from other products or after the reaction through evaporation, spillage, or other unavoidable losses.
05

Can a Reaction have 110% Actual Yield?

In general, a reaction cannot have an actual yield greater than 100% because this would mean that more product is being produced than is theoretically possible based on the balanced chemical equation. However, in certain cases, the actual yield might appear to be greater than 100% due to experimental errors or inaccuracies in measurement, leading to an incorrect calculation of the actual and/or theoretical yield. This is considered an anomaly and should be carefully checked for errors in the experiment or calculations.

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Most popular questions from this chapter

Write a balanced chemical equation for the reaction that occurs when (a) calcium metal undergoes a combination reaction with \(\mathrm{O}_{2}(g) ;\) (b) copper(II) hydroxide decomposes into copper(II) oxide and water when heated; (c) heptane, \(\mathrm{C}_{7} \mathrm{H}_{16}(l),\) burns in air; (d) methyl tert-butyl ether, \(\mathrm{C}_{5} \mathrm{H}_{12} \mathrm{O}(l)\) burns in air.

(a) When the metallic element sodium combines with the nonmetallic element bromine, \(\mathrm{Br}_{2}(l),\) how can you determine the chemical formula of the product? How do you know whether the product is a solid, liquid, or gas at room temperature? Write the balanced chemical equation for the reaction. (b) When a hydrocarbon burns in air, what reactant besides the hydrocarbon is involved in the reaction? What products are formed? Write a balanced chemical equation for the combustion of benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}(l),\) in air.

Washing soda, a compound used to prepare hard water for washing laundry, is a hydrate, which means that a certain number of water molecules are included in the solid structure. Its formula can be written as \(\mathrm{Na}_{2} \mathrm{CO}_{3} \cdot x \mathrm{H}_{2} \mathrm{O},\) where \(x\) is the number of moles of \(\mathrm{H}_{2} \mathrm{O}\) per mole of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\). When a \(2.558-\mathrm{g}\) sample of washing soda is heated at \(25^{\circ} \mathrm{C},\) all the water of hydration is lost, leaving \(0.948 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{CO}_{3} .\) What is the value of \(x ?\)

If \(1.5 \mathrm{~mol} \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}, 1.5 \mathrm{~mol} \mathrm{C}_{3} \mathrm{H}_{8},\) and \(1.5 \mathrm{~mol} \mathrm{CH}_{3} \mathrm{CH}_{2}\) \(\mathrm{COCH}_{3}\) are completely combusted in oxygen, which produces the largest number of moles of \(\mathrm{H}_{2} \mathrm{O} ?\) Which produces the least? Explain.

When a mixture of \(10.0 \mathrm{~g}\) of acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right) ;\) and \(10.0 \mathrm{~g}\) of oxygen \(\left(\mathrm{O}_{2}\right)\) is ignited, the resultant combustion reaction produces \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) (a) Write the balanced chemical equation for this reaction. (b) Which is the limiting reactant? (c) How many grams of \(\mathrm{C}_{2} \mathrm{H}_{2}, \mathrm{O}_{2}, \mathrm{CO}_{2},\) and \(\mathrm{H}_{2} \mathrm{O}\) are present after the reaction is complete?
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