Explanation

According to the Bronsted-Lowry theory, NH3 acts as a base because it can accept a proton (H^+).

According to the Lewis theory, NH3 is a base because it can donate a pair of electrons.

Explanation

According to the Arrhenius definition, an acid is a substance that increases the H+ ion concentration in aqueous solution.

HCl, HNO3, and H2SO4 all dissociate in water to produce H+ ions, making them Arrhenius acids.

CO2 does not dissociate in water to produce H+ ions.

Explanation

Preservatives are used to prevent the growth of microorganisms, such as bacteria, yeast, and mold, in food.

They help to extend the shelf life of food products and prevent spoilage.

Preservatives can be found in meats, dairy products, baked goods, and beverages.

Explanation

Acids are known to cause corrosive effects on skin, including burns, ulcers, and damage to skin tissue.

Examples of corrosive acids include sulfuric acid (H2SO4), hydrochloric acid (HCl), and nitric acid (HNO3).

Explanation

Important: Simply adding more product does not permanently increase Kc; it changes the reaction quotient until equilibrium is restored.

• Kc is the equilibrium constant.
• A larger Kc generally indicates equilibrium favors products.
• At equilibrium, the value of Kc depends on temperature.
• A catalyst does not change Kc.

Explanation

Qc (reaction quotient) is defined as the ratio of the molar concentrations of products to reactants, each raised to the power of their respective stoichiometric coefficients (coefficients in the balanced chemical equation).

Explanation

When the reaction quotient (Qc) is equal to the equilibrium constant (Kc), the system is at equilibrium and is stable.

Qc = Kc indicates that the rates of forward and reverse reactions are equal, and the concentrations of reactants and products remain constant.

Explanation

Explanation

• Kc is the equilibrium constant based on concentration.
• A small Kc means equilibrium favors the reactants.
• Therefore, more reactants remain at equilibrium.
• Only a small amount of products is formed.
• A large Kc  indicates that equilibrium favors the products.

Explanation

A reversible reaction is a reaction that can proceed in both the forward and reverse directions, and never goes to completion.

It is represented by a double arrow (⇌) between the reactants and products.

For example: A + B ⇌ C + D

Key Point:

• Single arrow (→): Represents an irreversible reaction, where the reaction only proceeds in one direction.