Kp Year 13 Chemistry

Kp is can be found for equilibrium mixtures of:

• Liquids

• Gases

• Heterogenous systems

• Solids

Mole fractions always have a value between:

• 0 and 1

• 0 and 100

Mole fraction is calculated by:

• Total moles − Moles at equilibrium

• Moles at equilibrium − Total moles

• Moles at equilibrium ÷ Total moles

• Total moles ÷ Moles at equilibrium

Partial pressure is found by:

• Mole fraction × Total pressure

• Mole fraction × Partial pressure

• Partial pressure ÷ 100

• Partial pressure × Total pressure

The partial pressures in a system always add up to:

• 100

• The total pressure

• 1

• 0

Which of these could NOT be a unit for partial pressure?

• Atm

• kPa

• Pa

• mol dm^-3

When pressure is measure in Pascals, Pa, what would be the units of the equilibrium constant, Kp, for the reaction shown?

• Pa²

• Pa^-1

• No units

• Pa^-2

When pressure is measure in atmospheres, atm, what would be the units of the equilibrium constant, Kp, for the reaction shown?

• atm

• No units

• atm^-2

• atm^-1

Kp is affected by:

• Concentration and pressure

• Temperature only

• The position of equilibrium

• Adding a catalyst

For the reaction shown, what are the effects when temperature is increased?

• Equilibrium shifts to the Left, Kp decreases

• Equilibrium shifts to the Left, Kp increases

• Equilibrium shifts to the Right, Kp increases

• Equilibrium shifts to the Right, Kp decreases