1.10 The Equilibrium Constant
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What is partial pressure ?
Each gas’ contribution to the total pressure
How do you calculate partial pressure of a gas ?
Partial pressure p = mole fraction x total pressure
What is a mole fraction ?
Mole fraction = moles of X / total moles in mixture
A reaction is represented by aA(g) + bB(g) ⇌ cC(g) + dD(g), what is Kp for the system ?
*Kp = (pCᶜ x pDᵈ) /( pAᵃ x pBᵇ) *pA = partial pressure of A *ᵃ = moles of A.
How do you calculate units for Kp ?
-Write out the units for partial pressure in the same arrangement as the Kp equation and cancel them out / multiply them -Usually in Pa, kPa or atm : do not change the units.
What is the effect of increasing temperature on Kp for an endothermic reaction ?
Equilibrium shifts to the right, so partial pressures of products increase, so Kp increases
What is the effect of increasing pressure on Kp in this reaction ? : Kp = (pCᶜ x pDᵈ) /( pAᵃ x pBᵇ)
Pressure does not affect Kp as moles of gas are the same on both sides
What will be the kinetic effect of increasing the temperature and pressure for any reaction ?
*Increasing both will increase the rate of reaction as : *Temperature increase results in many more particles having energy greater than Ea -> more successful collisions *Pressure - more particles in the same volume -> more successful collisions per second.