What equilibrium constant is used for gaseous equilibria based on partial pressures?
Kp
Kp is used when all species are gases and pressures are used instead of concentrations.
What quantity is used in the expression for Kp instead of concentration?
Partial pressure
Each gaseous species is represented by its partial pressure.
Fill in the blank:
Kp can only be used for equilibria occurring entirely in the _______ phase.
gas
Kp applies to homogeneous gas-phase equilibria.
True or False:
The value of Kp changes if the pressure of the system changes.
False
Changing pressure shifts equilibrium position but does not change Kp at constant temperature.
At what condition does the value of Kp remain constant?
Constant temperature
Equilibrium constants only change when temperature changes.
True or False:
Adding a catalyst changes the value of Kp.
False
Catalysts only speed up the attainment of equilibrium.
Fill in the blank:
The pressure exerted by one gas in a mixture is called its _______ pressure.
partial
It represents the contribution of that gas to the total pressure.
How can the partial pressure of a gas be calculated from mole fraction and total pressure?
Mole fraction × total pressure
Partial pressure = mole fraction × total pressure.
True or False:
The powers in a Kp expression correspond to the stoichiometric coefficients in the balanced equation.
True
The same rule used in Kc expressions also applies to Kp.
For the reaction aA + bB ⇌ cC + dD (all gases), how are products represented in the Kp expression?
Numerator
Kp = (PC)c(PD)d / (PA)a(PB)b.
Fill in the blank:
A large value of Kp indicates equilibrium lies mainly towards the _______.
products
Most reactants are converted into products at equilibrium.
What factor can change the value of Kp for a reaction?
Temperature
Changing temperature alters the equilibrium constant and equilibrium position.
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2.1 Atoms, Compounds, Molecules & Equations50
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2.2 Amount of Substance47
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2.3 Acid–Base69
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2.4 Electrons, Bonding and Structure90
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3.1 Periodicity22
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3.2 Group 2 and Halogens55
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3.3 Qualitative Analysis39
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3.4 Enthalpy Changes62
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3.5 Reaction Rates (Qualitative)55
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3.6 Equilibrium (Qualitative)24
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4.1 Basic Organic Chemistry Concepts42
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4.2 Hydrocarbons85
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4.3 Alcohols and Haloalkanes79
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4.4 Organic Synthesis12
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4.5 Analytical Techniques (IR & MS)36
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5.1 Reaction Rates (Quantitative)24
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5.2 Equilibrium (Quantitative)12
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5.3 pH and Buffers15
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5.4 Enthalpy, Entropy & Free Energy27
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5.5 Redox & Electrode Potentials63
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5.6 Transition Elements95
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6.1 Aromatic Compounds29
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6.2 Carbonyl Compounds20
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6.3 Carboxylic Acids & Esters25
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6.4 Nitrogen Compounds102
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6.5 Polymers24
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6.6 Organic Synthesis (Advanced)20
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6.7 Chromatography & Spectroscopy (NMR)26
