Gas Laws and Calculations

The video tutorial explains the preparation of ethine through the dehydration of ethanol using a solid catalyst. It describes the lab setup, the reaction process, and the collection of ethine gas. The tutorial also covers the calculation of the number of moles of ethine produced using the ideal gas law, considering the partial pressures of ethine and water. The video concludes with a calculation of the percent yield of ethine in the experiment.

What is the molar mass of ethine?

• 0.822 g/mol

• 35.7 g/mol

• 46.1 g/mol

• 28.1 g/mol

Which catalyst is used in the dehydration of ethanol?

• Liquid Catalyst

• Solid Catalyst

• Gas Catalyst

• No Catalyst

What was the volume of gas collected during the experiment?

• 0.200 L

• 1.000 L

• 0.500 L

• 0.854 L

At what temperature was the gas collected?

• 298 K

• 305 K

• 310 K

• 273 K

What is the ideal gas law formula used in the experiment?

• n = PV/RT

• V = nRT/P

• P = nRT/V

• PV = nRT

How is the partial pressure of ethine calculated?

• Total pressure minus vapor pressure of water

• Vapor pressure of water minus total pressure

• Total pressure plus vapor pressure of water

• Vapor pressure of water plus total pressure

What is the value of the gas constant R used in the calculations?

• 0.08206 L atm/mol K

• 0.0821 L atm/mol K

• 8.314 J/mol K

• 1.987 cal/mol K

What is the partial pressure of water at 305 K in atmospheres?

• 0.047 atm

• 0.822 atm

• 0.500 atm

• 0.775 atm

What is the total pressure during the experiment?

• 0.822 atm

• 1.000 atm

• 0.775 atm

• 0.500 atm

How many moles of ethine were produced in the experiment?

• 0.200 moles

• 0.150 moles

• 0.264 moles

• 0.300 moles