When heated with sulfuric or phosphoric acid, cyclohexanol, C6H11OH is converted to cyclohexene, C6H10. The balanced chemical equation for the reaction is shown below. C6H11OH(l) → C6H10 (l) + H2O(l) If the percent yield is 83%, what mass of cyclohexanol must we use to obtain 25 g of cyclohexene?

Question

When heated with sulfuric or phosphoric acid, cyclohexanol, C6H11OH is converted to cyclohexene, C6H10. The balanced chemical equation for the reaction is shown below. C6H11OH(l) → C6H10 (l) + H2O(l) If the percent yield is 83%, what mass of cyclohexanol must we use to obtain 25 g of cyclohexene?

Answer 1

Billions of kilograms of urea, are produced annually for use as a fertilizer. The reaction used is given below.

NH3(g) + CO2(g) → CO(NH2)2(s) + H2O(l)
The typical starting reaction mixture has a 3:1 mole ratio of NH3 to CO2. If 47.7 g urea forms per mole of that reacts, what is the

2.2.1. Theoretical yield;
2.2.2. Actual yield;
2.2.3. Percent yield?

Answer 2

To determine the mass of cyclohexanol needed to obtain 25 g of cyclohexene with an 83% yield, we need to use the concept of percent yield and stoichiometry.

Let's set up the equation to find the theoretical yield of cyclohexanol first:

1 mole of cyclohexene (C6H10) is produced from 1 mole of cyclohexanol (C6H11OH) based on the balanced chemical equation.
So, the molar mass of cyclohexene is 82.14 g/mol.

Now, let's calculate the theoretical yield of cyclohexanol:
Percent yield = (actual yield / theoretical yield) * 100
83% = (actual yield / theoretical yield) * 100
Theoretical yield = actual yield / (83/100)
Theoretical yield = 25 g / (83/100)
Theoretical yield = 25 g / 0.83
Theoretical yield = 30.1 g

The theoretical yield of cyclohexanol needed to obtain 25 g of cyclohexene is 30.1 g.

Answer 3

To determine the mass of cyclohexanol needed to obtain 25 g of cyclohexene with an 83% yield, we can use the concept of percent yield.

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

Theoretical yield is the maximum amount of product that can be obtained based on the balanced chemical equation.

In this case, from the balanced equation, we can see that the molar ratio of cyclohexanol to cyclohexene is 1:1. This means that for every 1 mole of cyclohexanol, we get 1 mole of cyclohexene.

The molar mass of cyclohexene is 82.15 g/mol, and since 25 g of cyclohexene is given, we can convert that to moles using the molar mass.

25 g cyclohexene * (1 mol cyclohexene / 82.15 g cyclohexene) = 0.304 moles cyclohexene

Since the molar ratio of cyclohexanol to cyclohexene is 1:1, the number of moles of cyclohexanol needed is also 0.304 moles.

Now, we can use the percent yield to calculate the mass of cyclohexanol:

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

83% = (actual yield / 0.304 moles) * 100

To solve for the actual yield, we rearrange the equation:

(actual yield / 0.304 moles) = 83% / 100

(actual yield / 0.304 moles) = 0.83

actual yield = 0.83 * 0.304 moles

Now, we can calculate the mass of cyclohexanol:

mass cyclohexanol = actual yield * molar mass cyclohexanol

mass cyclohexanol = (0.83 * 0.304 moles) * (100.16 g/mol)

mass cyclohexanol ≈ 25.14 g

Therefore, approximately 25.14 grams of cyclohexanol must be used to obtain 25 grams of cyclohexene with an 83% yield.

When heated with sulfuric or phosphoric acid, cyclohexanol, C6H11OH is converted to cyclohexene, C6H10. The balanced chemical equation for the reaction is shown below. C6H11OH(l) → C6H10 (l) + H2O(l) If the percent yield is 83%, what mass of cyclohexanol must we use to obtain 25 g of cyclohexene?

Billions of kilograms of urea, are produced annually for use as a fertilizer. The reaction used is given below.

m=30g

To determine the mass of cyclohexanol needed to obtain 25 g of cyclohexene with an 83% yield, we need to use the concept of percent yield and stoichiometry.

To determine the mass of cyclohexanol needed to obtain 25 g of cyclohexene with an 83% yield, we can use the concept of percent yield.