Practice Problem: Free Energy and Nonstandard Conditions

The video tutorial explains how to calculate the free energy change for a chemical reaction under non-standard conditions. It begins by introducing the reaction and the given non-standard conditions, such as temperature and pressure. The tutorial then explains why these conditions are non-standard and how they affect the free energy change. It provides a step-by-step guide to using the equation delta G = delta G° + RTlnQ, where Q is the reaction quotient. The tutorial concludes with the calculation of delta G, resulting in a value of 9.7 kJ/mol.

What is the standard free energy change for the given reaction?

• 50.0 kilojoules per mole

• 33.0 kilojoules per mole

• 40.0 kilojoules per mole

• 25.0 kilojoules per mole

Why are the given conditions considered non-standard?

• Because the conditions do not match standard temperature and pressure

• Because the temperature is above 100 degrees Celsius

• Because the reaction is at equilibrium

• Because the pressures of the gases are equal

Which formula is used to calculate the free energy change under non-standard conditions?

• Delta G = RTlnQ

• Delta G = Delta G° + RTlnQ

• Delta G = Delta G° + RTlnK

• Delta G = Delta H - T Delta S

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

• 8.314 joules per mole K

• 0.8314 joules per mole K

• 0.008314 kilojoules per mole K

• 8.314 kilojoules per mole K

What is the calculated free energy change for the reaction under the given non-standard conditions?

• 33.0 kilojoules per mole

• 9.7 kilojoules per mole

• 15.0 kilojoules per mole

• 23.3 kilojoules per mole