For many reactions, an increase of 10°C can double the reaction rate, so a 20°C increase typically results in the rate doubling.

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

According to Boyle's Law, at constant temperature, the volume of a gas decreases when the pressure increases due to compression.

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

According to Charles's Law, the volume of a gas increases with an increase in temperature at constant pressure.

According to Charles's Law, the volume of a gas increases with an increase in temperature at constant pressure.

Faraday's law states that the amount of substance deposited is proportional to the charge passed through the electrolyte.

Le Chatelier's principle states that if a system at equilibrium is subjected to a change, the system will adjust to counteract that change.

The bond angle in water is approximately 104.5 degrees due to the repulsion of the two lone pairs.

Bond order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (5 - 5) / 2 = 0.

Bond order = (number of bonding electrons - number of antibonding electrons) / 2. For 10 electrons, if all are bonding, bond order = 10/2 = 5. If 2 are antibonding, bond order = (10-2)/2 = 4. The most stable configuration gives a bond order of 2.

Bond order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (10 - 4) / 2 = 3.

Bond order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (3 - 1) / 2 = 1.

Bond order = (12 - 4) / 2 = 4. The bond order for O2 is actually 2, but this question is hypothetical.

N2 has 10 bonding electrons and 2 antibonding electrons, so bond order = (10 - 2) / 2 = 4 / 2 = 2.

O2 has 12 total valence electrons. The bond order is calculated as (number of bonding electrons - number of antibonding electrons) / 2 = (10 - 2) / 2 = 4 / 2 = 2.

O2 has 12 total electrons, with 10 in bonding orbitals and 2 in antibonding orbitals. Bond order = (number of bonding electrons - number of antibonding electrons) / 2 = (10 - 2) / 2 = 4 / 2 = 2.

In an endothermic reaction, heat is absorbed from the surroundings, resulting in a positive change in enthalpy (ΔH > 0).

In an exothermic reaction, heat is released, resulting in a negative change in enthalpy (ΔH < 0).

ΔH = Σ(bond enthalpies of reactants) - Σ(bond enthalpies of products) = [2(436) + 498] - [4(463)] = −572 kJ.

The change in enthalpy for the reaction is equal to the standard enthalpy of formation of H2O(l), which is -285.83 kJ/mol.

The change in enthalpy for the reaction is equal to the standard enthalpy of formation of H2O(l), which is -285.8 kJ/mol.

At constant pressure, the change in enthalpy (ΔH) is defined as the heat absorbed or released by the system.

The critical point is the temperature and pressure at which the gas and liquid phases of a substance become indistinguishable.

A catalyst increases the rate of both the forward and reverse reactions equally, thus it does not shift the equilibrium position but helps reach it faster.

A catalyst lowers the activation energy of a reaction, allowing it to proceed more quickly.

A catalyst speeds up the reaction rate without affecting the overall enthalpy change of the reaction.

According to the rate laws, increasing the concentration of reactants generally increases the rate of reaction, as it leads to more frequent collisions.

A catalyst speeds up the rate of both the forward and reverse reactions equally, thus having no effect on the position of the equilibrium.

Adding a strong acid increases the concentration of H+ ions, which can react with the weak base, shifting the equilibrium to the left to favor the formation of reactants.