Equilibrium Constants: Kc and Kp

This video tutorial explains the relationship between the equilibrium constants Kc and Kp, highlighting the differences in substances used for each. It derives the relationship using the ideal gas law equation PV=nRT and explains how to calculate Kp and Kc, including a practice problem. The video also discusses the conditions under which Kp equals Kc, emphasizing the role of Delta n in these calculations.

Which substances are included in the calculation of Kc?

• Solids and liquids

• Gases and aqueous solutions

• Liquids and gases

• Gases and solids

What is the primary difference between Kc and Kp?

• Kc includes solids, Kp includes liquids

• Kc measures concentrations, Kp measures pressures

• Kc is for liquids, Kp is for gases

• Kc and Kp are always equal

Which equation is used to relate Kc and Kp?

• E=mc^2

• F=ma

• V=IR

• PV=nRT

In the equation relating Kc and Kp, what does the term 'Delta n' represent?

• Change in volume

• Change in moles of gas

• Change in pressure

• Change in temperature

How is Delta n calculated?

• Initial moles minus final moles

• Moles of gaseous reactants minus moles of gaseous products

• Final moles minus initial moles

• Moles of gaseous products minus moles of gaseous reactants

What is the value of the gas constant R used in the Kc and Kp relationship?

• 0.08206 L·atm/mol·K

• 22.4 L

• 8.314 J/mol·K

• 1.00 atm

In the Kp expression, what is the exponent for the pressure of ammonia (NH3) if the coefficient is 2?

• 0

• 1

• 2

• 3

What is the value of Kp if the pressures of NH3, H2, and N2 are 0.418, 0.104, and 0.554 respectively?

• 418.104

• 0.337

• 2.80

• 280.337

What is the value of Delta n for the reaction if there are 2 moles of gaseous products and 4 moles of gaseous reactants?

• 2

• 0

• 4

• -2

Under what condition will Kp equal Kc?

• When Delta n is negative

• When Delta n is positive

• When Delta n is zero

• When Delta n is greater than one