For both roots to be positive, k must be greater than the square of half the coefficient of x: k > (6/2)^2 = 9.

The rate law for a reaction is determined experimentally and is dependent on the mechanism of the reaction.

The rate law for a reaction depends on the mechanism of the reaction.

The overall order of the reaction is the sum of the powers of the concentration terms, which is 1 + 2 = 3.

This is an example of Van 't Hoff rule, which states that the rate of reaction doubles for every 10°C increase in temperature.

The rate of reaction is expressed in terms of concentration change per unit time, hence the unit is mol/L·s.

This relationship is known as the rate law of the reaction.

Using Vieta's formulas, sum of roots = 1 + 2 = 3 = -(-4)/2 => k = 2*1*2 = 4.

Nucleotides are the building blocks of nucleic acids like DNA and RNA.

A large negative value of ΔG indicates that the reaction is highly spontaneous and favors the formation of products.

A negative ΔG indicates that the reaction is spontaneous under the given conditions.

A positive ΔG indicates that the reaction is non-spontaneous.

A positive ΔG indicates that the reaction is non-spontaneous.

A positive ΔS indicates an increase in disorder or randomness in the system.

A ΔG value of zero indicates that the reaction is at equilibrium, meaning the forward and reverse reactions occur at the same rate.

Raoult's Law states that the vapor pressure of a solvent in a solution is directly proportional to the mole fraction of the solvent.

The Gibbs free energy change indicates the spontaneity of a reaction; a negative value suggests spontaneity.

The enthalpy of reaction refers to the heat absorbed or released at constant pressure.

Entropy is a measure of the disorder or randomness in a system.

Gibbs free energy indicates the maximum reversible work that can be performed by a thermodynamic system at constant temperature and pressure.

For an endothermic reaction, increasing temperature generally decreases ΔG, making the reaction more favorable.

Increasing the concentration of a reactant in a first-order reaction increases the rate of the reaction.

The boiling point of a liquid decreases with a decrease in atmospheric pressure.

The boiling point of a solvent increases when a non-volatile solute is added due to boiling point elevation.

The entropy of a system increases when it undergoes an irreversible process.

When a reaction is reversed, the equilibrium constant for the reverse reaction is the reciprocal of the equilibrium constant for the forward reaction.

When a reaction is reversed, the equilibrium constant is inverted (1/K).

The freezing point of a solvent decreases when a non-volatile solute is added, a phenomenon known as freezing point depression.

The kinetic energy of particles increases as they gain energy to overcome intermolecular forces during melting.

According to Boyle's Law, if the volume is doubled at constant temperature, the pressure halves.