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.

The methoxy group (-OCH3) is an activating group and directs electrophilic substitution to the ortho and para positions.

A nitro group is a strong electron-withdrawing group that deactivates the benzene ring, making it less reactive towards electrophilic substitution.

A nitro group is a strong electron-withdrawing group that deactivates the benzene ring towards electrophilic substitution.

Strong electron-donating groups increase the electron density of the aromatic ring, enhancing its reactivity towards electrophiles.

A strong electron-withdrawing group decreases the reactivity of the benzene ring in electrophilic substitution by destabilizing the sigma complex.

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.

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

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

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.

Decreasing the volume increases the pressure, and according to Le Chatelier's Principle, the equilibrium will shift to the side with fewer moles of gas to counteract the change.

Decreasing the volume increases the pressure, shifting the equilibrium towards the side with fewer moles of gas. The left side has 2 moles (N2O) compared to 3 moles (N2 + O2), so it shifts to the left.

Hydrogen bonding significantly increases the boiling point of water compared to other similar-sized molecules.

Electronegativity decreases down a group because the increased distance between the nucleus and valence electrons reduces the nucleus's pull.

Increasing pressure shifts the equilibrium to the side with fewer moles of gas, which is the product side in this case.

According to Henry's Law, increasing pressure increases the solubility of a gas in a liquid.

The effect of temperature on cell potential depends on the reaction's enthalpy and entropy changes.

The effect of temperature on cell potential depends on the reaction's enthalpy and entropy changes.

Increasing temperature generally increases the enthalpy of an endothermic reaction as it favors the absorption of heat.

Increasing temperature generally increases the enthalpy of a substance due to increased kinetic energy.

For an exothermic reaction, increasing temperature shifts the equilibrium to the left, decreasing the equilibrium constant K.

According to the Arrhenius equation, an increase in temperature results in an exponential increase in the rate constant, thus increasing the reaction rate.

Increasing temperature increases the kinetic energy of molecules, leading to more frequent and effective collisions, thus increasing the reaction rate.

Increasing temperature generally increases the rate of an electrochemical reaction due to higher kinetic energy.

Increasing temperature generally decreases the solubility of gases, including hydrogen, in water.

Increasing the concentration of a product will shift the equilibrium to the left, favoring the formation of reactants, according to Le Chatelier's Principle.

Increasing the concentration of a reactant will require a greater volume of titrant to reach the equivalence point.