Increasing pressure raises the boiling point of a liquid.

Increasing temperature will make ΔG more negative for a reaction with a negative ΔH and positive ΔS, enhancing spontaneity.

For a reaction with ΔH > 0 and ΔS < 0, increasing temperature will make ΔG more positive, thus decreasing spontaneity.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants.

Increasing temperature generally decreases physisorption because it disrupts the weak van der Waals forces.

The effect of increasing temperature on cell potential depends on the reaction and its enthalpy change.

The effect of temperature on cell potential depends on the reaction and its enthalpy change.

Generally, the density of liquids decreases with an increase in temperature.

Increasing temperature generally increases the kinetic energy of particles, leading to greater disorder and thus an increase in entropy.

Increasing temperature generally increases the entropy of a system as the molecular motion becomes more chaotic.

For endothermic reactions, increasing temperature shifts the equilibrium to the right, increasing Kc.

For an endothermic reaction, increasing the temperature increases the equilibrium constant.

According to Le Chatelier's principle, increasing the temperature of an exothermic reaction shifts the equilibrium to the left, decreasing the equilibrium constant.

Increasing temperature increases the kinetic energy of gas molecules.

Increasing temperature increases the kinetic energy of gas particles.

Increasing temperature increases the kinetic energy of particles in a substance.

According to Gay-Lussac's law, pressure increases with temperature at constant volume.

Increasing temperature generally increases the rate of a chemical reaction.

For most solid solutes, increasing temperature increases solubility in water.

Increasing temperature increases the kinetic energy of the molecules, leading to an increase in vapor pressure.

Increasing temperature generally increases the vapor pressure of a solution due to increased kinetic energy of the molecules.

Increasing temperature generally increases the vapor pressure of a solvent, as more molecules have enough energy to escape into the vapor phase.

Increasing temperature generally decreases the viscosity of a liquid.

Increasing the carbon chain length generally decreases the acidity of carboxylic acids due to the inductive effect.

The boiling point of aldehydes increases with the increase in carbon chain length due to increased van der Waals forces.

In a first-order reaction, increasing the concentration of a reactant results in a linear increase in the rate.

Increasing the concentration of a solute lowers the freezing point of a solution.

Increasing the concentration of reactants generally increases the rate of a reaction.

Increasing the distance from the pivot point increases the torque produced by the force.

Increasing the number of alkyl substituents on the double bond increases the stability of alkenes due to hyperconjugation.