The work done by the system at constant pressure is given by W = PΔV, where P is pressure and ΔV is the change in volume.

The coordination number refers to the number of ligands that are directly bonded to the central metal ion in a coordination complex.

In a Daniell cell, the zinc electrode acts as the anode where oxidation occurs, releasing electrons.

In a Daniell cell, Cu²⁺ is reduced to Cu at the cathode.

For a first-order reaction, the half-life (t1/2) is given by t1/2 = 0.693/k. Rearranging gives k = 0.693/t1/2 = 0.693/10 min = 0.0693 min^-1.

For a first-order reaction, the half-life is independent of the initial concentration. Therefore, it remains 10 minutes.

For a first-order reaction, the half-life is independent of concentration. Therefore, the half-life remains 10 minutes.

Sodium ions produce a characteristic bright yellow color when subjected to a flame test.

In a galvanic cell, reduction occurs at the cathode, where electrons are gained.

In a galvanic cell, oxidation occurs at the anode, where electrons are released.

A triple bond consists of 1 sigma bond and 2 pi bonds.

The solvent can influence the reaction rate by stabilizing the transition state and the reactants involved in the nucleophilic substitution.

The line between the solid and liquid phases in a phase diagram represents the melting point, where solid and liquid coexist.

The Rf value is primarily affected by the polarity of the solvent used in paper chromatography, as it influences the interaction between the stationary phase and the analyte.

Adding an inert gas at constant volume does not change the partial pressures of the reactants or products, thus having no effect on the equilibrium position.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants, as the system absorbs heat.

According to Le Chatelier's principle, increasing the concentration of a reactant shifts the equilibrium to the right, favoring product formation.

Increasing the pressure by decreasing the volume shifts the equilibrium towards the side with fewer moles of gas, according to Le Chatelier's Principle.

Increasing the volume decreases the pressure, which shifts the equilibrium towards the side with more moles of gas.

At equilibrium, the concentrations of reactants and products remain constant over time.

For endothermic reactions, increasing temperature shifts the equilibrium and increases enthalpy.

If the number of moles of gas is equal on both sides, increasing the pressure has no effect on the equilibrium position.

An intermediate is a species that is formed during the reaction and consumed in subsequent steps, not appearing in the overall reaction.

An intermediate is a species that is produced in one step of a reaction mechanism and consumed in a later step.

The rate-determining step is the slowest step in a reaction mechanism and thus controls the overall rate of the reaction.

Decreasing the temperature in an endothermic reaction shifts the equilibrium to the left, favoring the formation of reactants as the system seeks to release heat.

Decreasing the temperature in an endothermic reaction shifts the equilibrium to the left, favoring the formation of reactants as the system seeks to release heat.

Using the Arrhenius equation and the temperature dependence of the rate constant, Ea can be estimated using the formula Ea = (R * ΔT * ln(2)) / (1/T1 - 1/T2). For a 10°C increase, Ea is approximately 80 kJ/mol.

For a first-order reaction, t = (ln([A]0/[A]) / k). Here, [A] = 0.25[A]0, so t = (ln(1/0.25) / 0.03) ≈ 46.2 s.

The change from +7 to +2 indicates a gain of 5 electrons (7 - 2 = 5).