Calculating Alcohol Dehydration Yields: 2-Methylcyclohexanol To 2-Methylcyclohexene

The theoretical yield of a chemical reaction refers to the maximum amount of product that can be obtained under ideal conditions. In the context of alcohol dehydration, specifically the dehydration of 2-methylcyclohexanol (C7H14O), the theoretical yield can be calculated through a series of steps. The molecular weight of 2-methylcyclohexanol, its density, and the specified volume are all factors used in the calculation. By converting the volume to litres and applying the density formula, the mass of 2-methylcyclohexanol can be determined. This mass value is then used in conjunction with the molecular weight to calculate the theoretical yield in grams, providing an estimate of the maximum amount of product that can be obtained from the dehydration reaction.

Dehydration reaction formula: C7H14O → C7H12 + H2O

Dehydration reactions involve the removal of water (H2O) from a substance. In the context of alcohol dehydration, oxygen is removed from the alcohol molecule in the form of water, resulting in the formation of an olefin or alkene. This is represented by the balanced equation: C7H14O → C7H12 + H2O, which indicates that one mole of alcohol yields one mole of alkene and one mole of water.

To calculate the theoretical yield of the dehydration reaction for 4.00 mL of 2-methylcyclohexanol (C7H14O), we can follow these steps: First, we need to determine the molecular weight of 2-methylcyclohexanol, which is given by its molecular formula, C7H14O. The molecular weight is calculated by summing the atomic weights of carbon, hydrogen, and oxygen atoms in the molecule. In this case, the molecular weight of 2-methylcyclohexanol is 106 g/mol.

Next, we convert the volume of 4.00 mL to litres, which gives us 0.004 L. We can then use the equation mass = volume x density to find the mass of 2-methylcyclohexanol used. The density of 2-methylcyclohexanol is 0.841 g/mL, so the mass of 0.004 L is 0.841 g/mL x 0.004 L, which equals 0.00336 g.

Now that we have the mass and molecular weight of 2-methylcyclohexanol, we can calculate the theoretical yield using the equation yield = mass/molecular weight. Plugging in the values, we get 0.00336 g/106 g/mol, which gives us a theoretical yield of approximately 3.17 x 10^-5 grams or 3.17E-5 g.

Alternatively, we can calculate the theoretical yield by first determining the number of moles of alkene produced. Since the balanced equation tells us that one mole of alcohol yields one mole of alkene, the moles of alkene produced are equal to the moles of 2-methylcyclohexanol used. Given the mass of 2-methylcyclohexanol (0.00336 g) and its molecular weight (106 g/mol), we can calculate the moles using the formula moles = mass/molecular weight. This gives us approximately 0.0294 mol.

Finally, to find the theoretical yield in grams, we multiply the moles of alkene produced by its molar mass. The alkene produced in this reaction is likely 2-methylcyclohexene (C7H12), which has a molar mass of 84.16 g/mol. Therefore, theoretical yield = moles of alkene × molar mass of alkene, which is approximately 0.0294 mol × 84.16 g/mol = 2.475 grams.

In conclusion, the theoretical yield of the dehydration reaction for 4.00 mL of 2-methylcyclohexanol is approximately 2.475 grams or 2.5 x 10^-3 grams. This calculation assumes complete conversion of the reactant to the product and provides an ideal yield without considering experimental losses or impurities.

1 mole of alcohol yields 1 mole alkene

The dehydration reaction of 2-methylcyclohexanol can be simplified to the following equation: C7H14O → C7H12 + H2O. This equation illustrates the loss of a water molecule, resulting in the conversion of an alcohol to an alkene.

In this reaction, 1 mole of alcohol yields 1 mole of alkene and 1 mole of water. This stoichiometric relationship is fundamental to understanding the reaction's outcome. The balanced equation tells us that for every mole of 2-methylcyclohexanol (C7H14O) consumed, one mole of 2-methylcyclohexene (C7H12) is produced, along with one mole of water (H2O).

To calculate the theoretical yield of the dehydration reaction for a given amount of 2-methylcyclohexanol, you would follow these steps: First, determine the mass of 2-methylcyclohexanol present. This can be done by multiplying the volume (in litres) by the density (in g/mL). Then, using the molecular weight of 2-methylcyclohexanol (106 g/mol), you can calculate the moles of 2-methylcyclohexanol. This value represents both the moles of alkene produced and the moles of water generated in the reaction. Finally, to find the theoretical yield in grams, multiply the moles of alkene by the molar mass of the alkene (84.16 g/mol).

For example, let's consider the dehydration reaction of 4.00 mL of 2-methylcyclohexanol. The mass of 2-methylcyclohexanol is calculated as 0.841 g/mL (density) × 0.004 L (volume) = 0.00336 g. The moles of 2-methylcyclohexanol are then calculated as 0.00336 g/106 g/mol = 0.0294 mol. This is also the number of moles of alkene produced. Finally, the theoretical yield is calculated as 0.0294 mol × 84.16 g/mol ≈ 2.475 g.

In conclusion, the statement "1 mole of alcohol yields 1 mole of alkene" is a fundamental concept in the dehydration of alcohols to alkenes. This 1:1 stoichiometric ratio is evident in the balanced equation and forms the basis for calculating the theoretical yield of alkene in dehydration reactions.

Molecular weight of 2-methylcyclohexanol: 106 g/mol

The molecular weight of 2-methylcyclohexanol is 106 g/mol. This is calculated from its molecular formula, C7H14O.

To determine the theoretical yield of the dehydration reaction of 2-methylcyclohexanol, we can use this molecular weight. The balanced equation for the dehydration of 2-methylcyclohexanol is given as: C7H14O → C7H12 + H2O. This equation tells us that one mole of alcohol yields one mole of alkene and one mole of water.

Now, let's assume we have 4.00 mL of 2-methylcyclohexanol. We can convert this volume to litres (0.004 L) and then calculate the mass of 2-methylcyclohexanol used. The density of 2-methylcyclohexanol is 0.841 g/mL, so the mass is 0.841 g/mL x 0.004 L, which equals 0.00336 g.

Using the molecular weight of 106 g/mol, we can calculate the theoretical yield by dividing the mass by the molecular weight: 0.00336 g/106 g/mol, which is approximately 3.17 x 10^-5 grams or 0.0000317 grams.

Therefore, the theoretical yield of the dehydration reaction of 4.00 mL of 2-methylcyclohexanol is approximately 3.17 x 10^-5 grams.

Theoretical yield formula: Moles of alkene x Molar mass of alkene

To calculate the theoretical yield of a reaction, you need to determine the mass of the reactants required to produce a certain mass of the desired product. This can be achieved using the theoretical yield formula, which involves finding the moles of the limiting reagent and applying stoichiometry.

In the case of the dehydration reaction of 2-methylcyclohexanol (C7H14O), the balanced equation is: C7H14O → C7H12 + H2O. This equation tells us that one mole of 2-methylcyclohexanol yields one mole of alkene (likely 2-methylcyclohexene, C7H12) and one mole of water. Therefore, to calculate the theoretical yield of alkene, we need to determine the moles of 2-methylcyclohexanol used in the reaction.

Let's assume we have 4.00 mL of 2-methylcyclohexanol. First, we convert the volume to liters (0.004 L). Then, we can calculate the mass of 2-methylcyclohexanol using the formula mass = volume x density. With a density of 0.841 g/mL, the mass of 2-methylcyclohexanol is 0.00336 g.

Now that we have the mass, we can calculate the moles of 2-methylcyclohexanol using its molar mass (106 g/mol). This gives us 0.0294 mol. Since the reaction produces one mole of alkene for every mole of 2-methylcyclohexanol, the moles of alkene produced are also 0.0294 mol.

Finally, to find the theoretical yield in grams, we multiply the moles of alkene by the molar mass of the alkene (84.16 g/mol for 2-methylcyclohexene). This gives us a theoretical yield of approximately 2.475 grams.

In summary, the theoretical yield formula involves calculating the moles of the limiting reagent (in this case, 2-methylcyclohexanol) and then multiplying it by the molar mass of the desired product (the alkene). This allows us to determine the maximum amount of product that could be obtained based on stoichiometry.

Theoretical yield for 4.00ml: 2.475 grams

To calculate the theoretical yield for the dehydration reaction of 4.00 mL of 2-methylcyclohexanol, we can follow these steps:

First, we need to understand the chemical equation for the dehydration of 2-methylcyclohexanol. The balanced equation is given as C7H14O → C7H12 + H2O, which indicates that one mole of alcohol yields one mole of alkene and one mole of water.

Now, let's calculate the number of moles of 2-methylcyclohexanol present in 4.00 mL. To do this, we need to know the density of 2-methylcyclohexanol, which is 0.841 g/mL. So, the mass of 4.00 mL of 2-methylcyclohexanol is 0.841 g/mL x 0.004 L, which equals 0.00336 grams.

Next, we can find the number of moles by dividing the mass by the molecular weight of 2-methylcyclohexanol, which is 106 g/mol. This gives us approximately 0.0294 moles.

Finally, to find the theoretical yield in grams, we multiply the number of moles by the molar mass of the alkene produced (likely 2-methylcyclohexene, C7H12) which has a molecular weight of 84.16 g/mol. So, the calculation is 0.0294 mol x 84.16 g/mol, resulting in approximately 2.475 grams.

Therefore, the theoretical yield for the dehydration reaction of 4.00 mL of 2-methylcyclohexanol is 2.475 grams. This calculation assumes a complete reaction with 100% yield, hence the term "theoretical yield."

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