Chemical Equilibrium Principles Quiz

M. C. Chidambaram, V. S. Veeramani, and M. A. Parasaratty started the "Sip and Learn" sessions to teach chemical equilibrium.
Chemical equilibrium refers to a physical state where the forward reaction and the reverse reaction occur at equal rates.
Physical meaning of chemical equilibrium: The reactants and products have equal concentrations.
Homogeneous chemical equilibrium: Both the reactants and products are in the same phase.
For example, if a reaction has two reactants, A and B, and two products, C and D, the equilibrium constant, Kc, can be calculated by the equation: Kc = ([C] * [D]) / ([A]^2 * [B]^2)
Kc represents the position of equilibrium.
The forward reaction rate is the product of the concentration of reactants and their respective reaction orders raised to the power of their coefficients.
The reverse reaction rate is the product of the concentration of products and their respective reaction orders raised to the power of their coefficients.
When the forward and reverse reaction rates are equal, the system is at equilibrium.
If the reactants are being added or the products are being removed, the system will move towards the new equilibrium until the system reaches the new equilibrium state.
The temperature effect on equilibrium: An increase in temperature favors the reaction with a larger positive enthalpy change (endothermic) and decreases the reaction with a larger negative enthalpy change (exothermic).
The pressure effect on equilibrium (for gases): An increase in pressure favors the reaction with a larger number of moles of gas formed.
The rate of a reaction depends on the concentrations of the reactants and the temperature.
The reaction rate equation is given by the rate = k[A]^m[B]^n, where A and B are the reactants, k is the rate constant, m and n are the reaction orders of A and B respectively.
The reaction rate constant is a measure of the reaction rate at a given temperature and concentration.
Catalysts increase the rate of a reaction by lowering the activation energy, not by providing energy.
The position of equilibrium is influenced by the temperature, concentration, and presence of a catalyst.
Equilibrium can be represented graphically using a reaction coordinate diagram, which plots the energy of the reactants and products against the reaction progress.
Le Chatelier's principle states that when a stress (change in concentration, temperature, or pressure) is applied to a system at equilibrium, the system responds by shifting the equilibrium in a direction that minimizes the stress.
Equilibrium constants can be related to each other through the Legendre transformation, which is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
Equilibrium constants can be calculated using various experimental methods, such as titration, calorimetry, and spectrophotometry.
The equilibrium constant and the position of equilibrium are related through the equation: Kc = [C]eq[D]eq / [A]eq^2[B]eq^2, where [C]eq, [D]eq, [A]eq, and [B]eq are the concentrations of the reactants and products at equilibrium.
The pressure-volume product (PVn) of a system is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature. It is related to the equilibrium constant through the equation: PVn = nRTlnKc, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
The equilibrium constant can be used to calculate the equilibrium constant for a reaction at different temperatures and pressures.
The position of equilibrium for a reaction can be determined by measuring the concentrations of the reactants and products at equilibrium.
The equilibrium constant for a reaction can be determined by measuring the reaction rate at different concentrations and temperatures and using the rate constant and the reaction order information.
The equilibrium constant for a reaction can be calculated from the experimental data using the equilibrium constant expression and the concentrations of the reactants and products at equilibrium.
The equilibrium constant for a reaction can be calculated from the free energy change (ΔG) using the equation: Kc = e^(ΔG° / RT), where ΔG° is the standard free energy change and R is the gas constant.
The equilibrium constant for a reaction can be calculated from the enthalpy change (ΔH) and the entropy change (ΔS) using the equation: Kc = e^(ΔH° / RT) × e^(ΔS° / R), where ΔH° and ΔS° are the standard enthalpy and entropy changes respectively.
The equilibrium constant for a reaction can be calculated from the Gibbs free energy change (ΔG) using the equation: Kc = e^(ΔG° / RT), where ΔG° is the standard Gibbs free energy change and R is the gas constant.
The equilibrium constant for a reaction can be calculated from the reaction quotient (Q) using the equation: Kc = Q.
The equilibrium constant for a reaction can be calculated from the initial and final concentrations of the reactants and products using the equation: Kc = [C]f / [A]i^m[B]i^n, where [C]f is the concentration of the product at equilibrium, [A]i and [B]i are the initial concentrations of the reactants, and m and n are the reaction orders of A and B respectively.
The equilibrium constant for a reaction can be calculated from the initial and final volumes of the gases involved in the reaction using the equation: Kc = (P2 / P1)n, where P1 and P2 are the initial and final pressures of the gases and n is the number of moles of gas involved in the reaction.
The equilibrium constant for a reaction can be calculated from the initial and final masses of the reactants and products using the equation: Kc = (m2 / m1)n, where m1 and m2 are the initial and final masses of the reactants and products and n is the number of moles of the reactants and products involved in the reaction.
The equilibrium constant for a reaction can be calculated from the initial and final temperatures using the equation: Kc = T2 / T1, where T1 and T2 are the initial and final temperatures.
The equilibrium constant for a reaction can be calculated from the initial and final energies using the equation: Kc = E2 / E1, where E1 and E2 are the initial and final energies.
The equilibrium constant for a reaction can be calculated from the initial and final enthalpies using the equation: Kc = H2 / H1, where H1 and H2 are the initial and final enthalpies.
The equilibrium constant for a reaction can be calculated from the initial and final entropy using the equation: Kc = S2 / S1, where S1 and S2 are the initial and final entropies.
The equilibrium constant for a reaction can be calculated from the initial and final Gibbs free energies using the equation: Kc = Γ2 / Γ1, where Γ1 and Γ2 are the initial and final Gibbs free energies.
The equilibrium constant for a reaction can be calculated from the initial and final free energies of activation using the equation: Kc = ΔGact2 / ΔGact1, where ΔGact1 and ΔGact2 are the initial and final free energies of activation.
The equilibrium constant for a reaction can be calculated from the initial and final reaction rates using the equation: Kc = vf / vi, where vf and vi are the initial and final reaction rates.
The equilibrium constant for a reaction can be calculated from the initial and final concentrations of the reactants and products using the equation: Kc = [C]f / [A]i^m[B]i^n, where [C]f is the concentration of the product at equilibrium, [A]i and [B]i are the initial concentrations of the reactants, and m and n are the reaction orders of A and B respectively.
The equilibrium constant for a reaction can be calculated from the initial and final volumes of the gases involved in the reaction using the equation: Kc = (P2 / P1)n, where P1 and P2 are the initial and final pressures of the gases and n is the number of moles of gas involved in the reaction.
The equilibrium constant for a reaction can be calculated from the initial and final masses of the reactants and products using the equation: Kc = (m2 / m1)n, where m1 and m2 are the initial and final masses of the reactants and products and n is the number of moles of the reactants and products involved in the reaction.
The equilibrium constant for a reaction can be calculated from the initial and final temperatures using the equation: Kc =