The longest chain has 4 carbons with a carboxylic acid group, making it 2-methylbutanoic acid.

The correct IUPAC name for CH3-CH2-CH(CH3)-OH is 2-Methyl-1-propanol, as the longest chain has three carbons and the hydroxyl group is on the first carbon.

The longest carbon chain has four carbons and the hydroxyl group is on the first carbon, making it Butan-1-ol.

The longest carbon chain has four carbons with an aldehyde group, making it 2-Methylbutanal.

The longest chain has four carbons, and there is a methyl group on the second carbon, making it 2-methylbutane.

The compound is 2-methylbutanoic acid, as the carboxylic acid is on the second carbon of the butane chain.

The longest chain has five carbons (pentane) with two methyl groups on the third carbon, making it 3,3-dimethylpentane.

The longest chain has five carbons, and the methyl group is on the third carbon, making it 3-methylpentane.

The compound has three carbon atoms in the longest chain and a carboxylic acid functional group, making it propanoic acid.

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.

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.

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

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.

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.

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.

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.

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

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

An increasing electronegativity difference leads to greater ionic character in the bond, making it more polar.