The relationship between Kp and Kc is given by Kp = Kc(RT)^(Δn), where Δn = (d+c) - (a+b).

The relationship is given by the equation pKa = -log(Ka), where Ka is the acid dissociation constant.

The relationship is given by the formula pKa = -log(Ka), where Ka is the acid dissociation constant.

The relationship is given by pKa = -log(Ka), where Ka is the acid dissociation constant.

Pressure and temperature are directly proportional for a fixed amount of gas at constant volume, as described by Gay-Lussac's law.

Gay-Lussac's Law states that pressure is directly proportional to temperature when volume is constant.

The kinetic energy of gas molecules is directly proportional to the temperature.

The kinetic energy of gas molecules is directly proportional to the temperature of the gas.

The rate of a chemical reaction generally increases with an increase in temperature due to higher kinetic energy.

At constant temperature and pressure, density is directly proportional to molar mass according to the ideal gas law.

The relationship is given by the equation ΔG = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin.

At equilibrium, the reaction quotient Q is equal to the equilibrium constant K.

The relationship between Kp and Kc is given by Kp = Kc(RT)^(Δn), where Δn is the change in the number of moles of gas.

The relationship is given by the equation ΔG = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin.

ΔG = -RT ln K relates Gibbs free energy change to the equilibrium constant.

Boiling point elevation is directly proportional to the molality of the solution.

In a hydrogen atom, the energy of an electron increases with increasing principal quantum number (n).

The relationship is given by ΔG = -RT ln K, where R is the gas constant and T is temperature.

The relationship is given by ΔG = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin.

The relationship is given by the equation ΔG = ΔH - TΔS, where T is the temperature in Kelvin.

At equilibrium, the change in Gibbs free energy (ΔG) is zero.

At constant pressure, the relationship is given by ΔH = ΔU + PΔV.

A catalyst speeds up the reaction without being consumed in the process.

The salt bridge maintains charge balance by allowing ions to flow between the two half-cells.

Activated charcoal is commonly used as an adsorbent due to its high surface area and porosity.

In an electrochemical cell, reduction occurs at the cathode.

AX3E indicates three bonding pairs and one lone pair, resulting in a trigonal pyramidal shape.

Ammonia has a trigonal pyramidal shape due to the presence of a lone pair on the nitrogen atom.

The d orbitals have a double dumbbell shape.

π bonds are formed by the side-to-side overlap of p orbitals, resulting in a planar shape.