Ethylene Production and Yield Calculations

The video tutorial explains how to calculate the number of moles of ethine produced from ethanol in a dehydration reaction. It covers the conversion of ethanol mass to moles, the theoretical yield of ethine if the reaction goes to completion, and the calculation of the percent yield based on experimental data.

What is the initial mass of ethanol used in the reaction?

• 2 g

• 0.02 kg

• 0.02 g

• 0.2 g

What is the molar mass of ethanol used in the calculation?

• 46.1 g/mol

• 44.1 g/mol

• 50.1 g/mol

• 48.1 g/mol

How many moles of ethanol are present in 0.2 g of ethanol?

• 0.000434 moles

• 0.434 moles

• 0.0434 moles

• 0.00434 moles

If the reaction goes to completion, how many moles of ethine are produced from 0.434 moles of ethanol?

• 0.0434 moles

• 4.34 moles

• 0.434 moles

• 0.00434 moles

What is the actual number of moles of ethine obtained in the experiment?

• 0.264 moles

• 0.434 moles

• 0.00434 moles

• 0.034 moles

What is the formula for calculating percent yield?

• (Theoretical yield - Actual yield) x 100

• (Actual yield + Theoretical yield) x 100

• (Theoretical yield / Actual yield) x 100

• (Actual yield / Theoretical yield) x 100

What is the percent yield of ethine in the experiment?

• 60.8%

• 68.0%

• 80.6%

• 86.0%

Why is the actual yield of ethine less than the theoretical yield?

• The reaction was at a high temperature

• The reaction was too slow

• The reaction was too fast

• The reaction did not go to completion

What is the significance of using significant figures in the calculation?

• To ensure precision

• To make calculations easier

• To reduce errors

• To increase the number of decimals

What is the relationship between moles of ethanol and moles of ethine in the reaction?

• 3:1

• 1:1

• 2:1

• 1:2