A5 Equilibria
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Using Le Chatalier’s principale explain the effect of increasing temperature
• Forwards reaction is exo/endothermic • So increasing temperautre favours forwards/backwards reaction • Equilibrium concentration of XXX increases
Define dynamic equilibria
• Exists only in a closed system • The rate of the forward reaction is equal to the rate of the reverse reaction • The concentrations of reactants and products do not change
Using Le Chatalier’s principale explain the effect of increasing pressure
• Fewer gas moles on the left/right • Increasing pressure shifts equallibrium to the left/right hand side • Equilibrium concentration of XXX incresaes
Using Le Chatalier’s principale explain the effect of increasing concentration of reactants
• More reactant particles in mixture per unit volume • Equilibrium shifts to right hand side
Using Le Chatalier’s principale explain the effect of a catalyst
• Increases the rate of both the forwards and backwards reactions in the equilibria by the same ammount • The position of equalibria remains unchanged
In equilibria industry, what are the advantageous/disadvantages to temperature
• High temperature = quicker rate • High temperature is expensive
In equilibria industry, what are the advantageous/disadvantages to pressure
• High pressure = quicker rate • High pressure = expensive • High pressure = dangerous
Why is it difficult to know the effect on equalibria if it is affected by both temperature and pressure
Difficult to predict relative contributions of two opposing factors
Why is nitrogen accesible in industry
Occurs naturally in the air
Explain the effect of changing temperature on the position of Kc
• If temperature change causes equilibria to shift to the right hand side, Kc value increases • If temperature change causes equilibria to shift to the left hand side, Kc value decreases • Kc value is not affected by pressure, or catalysts
Stages required for Kc with brief explaination of each one if applicable
• Initial moles • Change in moles (use molar ratio, and oppostie sides of the equation are positive and negative) • Equilibrium moles • Concentration (Conc=mol/vol)
What should always be ignored in Kc calculations
Solids
Stages for calculating Kp with a brief explaination of each one if applicaible
• Initial moles • Change in moles (use molar ratio and opposite sides of equation have opposite signs) • Equilibrium moles • Mole fraction (E moles over total moles) • Partial pressure (multiply by volume)
What reactants and products should only be used in a Kp calculations
Gases only
Explain the effect of increasing pressure (causing right hand shift) on the Kp equation
• Equallibrium shifts right, as right hand side has fewer moles • Increased pressure results in denominator of Kp experssion increasing more than numerator • Numerator expression must increase to restore Kp
Explain how increasing temperature affects the value of Kp
• If temperature change causes equalibira to shift to right hand side, Kp value increases • If temperature change causes equalibira to shift to left hand side, Kp value decreases • Kp value is not affected by pressure, or catalysts