In the presence of an acid catalyst, cyclohexanol (100.16 g/mol) is dehydrated to give cyclohexane (82.14 g/mol) and water. A dehydration reaction starting with 3.3 g cyclohexanol produces 2.4 g cyclohexene. Calculate the theoretical yield for this reaction. Report your answer with two significant figures.

3.3 g cyclohexanol would theoretically produce 2.71g cyclohexene.

Explanation:

A theoretical yield is the amount of products created by a chemical reaction, provided none of the reactants were wasted and the reaction was fully completed.

Let's write out the balanced chemical equation for the reaction;

Cyclohexanol  --> Cyclohexane + Water

HOCH(CH2)5 --> C6H10 + H2O

Step 1: Determine the number of moles of each reactant

Number of moles = Mass/ molar mass = 3.3 / 100.16 = 0.03295 mol

From the equation; 1 mole of cyclohexanol produces 1 mol of cyclohexene.

This means 0.03295 mol of cyclohexanol produces 0.03295 mol of cyclohexene.

Mass of cyclohexene produced; Mass = Number of moles * Molar mass = 0.03295 * 82.14 = 2.71g

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answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :