mcqs of chemical equilibrium

Chemical Equilibrium MCQs with Answers

For students getting ready for their first academic exams in the Army, Navy, and Pakistan Air Force, multiple-choice questions on chemical equilibrium mcqs with answers are a great resource. These chemical equilibrium multiple-choice questions (MCQs) address many different aspects of equilibrium, including the crucial field of mathematics.

They are essential to the PN Cadets’ academic assessments in mathematics as well as the exams administered by the Navy Supply Branch, Navy Operation Branch, and Navy Operation Branch. These chemical equilibrium multiple-choice questions (MCQs) improve problem-solving abilities while offering a thorough comprehension of equilibrium principles. Aspiring candidates can ace their exams and establish a solid foundation in chemical equilibrium by using these practice problems.

Chemical Equilibrium MCQ (Part-1)

  • According to the law of mass action, the rate of a chemical reaction is directly proportional to the ________ of the reactants. (concentration)
  • The law of mass action is based on the principle ________. (chemical equilibrium)
  • The law of mass action applies to reactions that are _________. (reversible)
  • The law of mass action was formulated by ________ and ________. (Cato Guldberg and Peter Waage)
  • The law of mass action can be expressed mathematically using the equation ________. (rate)
  • According to the law of mass action, the rate of a reaction is proportional to the ________ of the reactants raised to their ________ power. (concentration, stoichiometric coefficients)
  • The law of mass action is a fundamental concept in the field of ________. (chemical kinetics)
  • The law of mass action can be applied to both ________ and ________ reactions. (homogeneous, heterogeneous)
  • The law of mass action can determine the ________ of a chemical reaction at a given temperature. (equilibrium constant)
  • The law of mass action assumes that a reaction occurs through a ________ mechanism. (elemental matter)
  • The law of mass action is used to predict the ________ of a reaction under different conditions. (rate)
  • The law of mass action can be modified by the presence of ________ or ________ in the reaction mixture. (catalysts, inhibitors)
  • The law of mass action is a basic principle in the field of ________. (chemical thermodynamics)

Chemical Equilibrium MCQ Questions with Answers

Chemical Equilibrium MCQ questions and answers are a crucial preparation resource for prospective candidates hoping to enter the Navy Ordnance Branch, Navy Weapon Engineering Branch, or Navy Education Branch.

In addition to covering the fundamental ideas of equilibrium, these chemical equilibrium multiple-choice questions also include mathematical elements that are essential to each branches’ scholastic examinations. Candidates can improve their performance on Navy exams and solidify their grasp of equilibrium principles by working through these multiple-choice questions.

Chemical Equilibrium MCQ (Part-2)

  • The law of mass action is based on the concept ________ that the speed of a chemical reaction depends on the frequency of collisions and the energy of the colliding particles. (collision theory)
  • The law of mass action gives a quantitative relationship between the ________ and ________ of a chemical reaction. (rate, concentration)
  • The equilibrium constant (K) is a measure of the ________ of a chemical reaction at a given temperature. (range)
  • The equilibrium constant (K) determines the ________ of a reaction. (stoichiometry)
  • The equilibrium constant (K) is defined as the ratio of products ________ to reactants ________ multiplied by the corresponding stoichiometric coefficients. (concentrations)
  • The equilibrium constant (K) is ________. (dimensionless)
  • The equilibrium constant (K) is expressed as a ________ expression. (mathematical)
  • The equilibrium constant (K) is denoted by the capital letter ________. (K)
  • The equilibrium constant (K) is related to the reaction coefficient (Q) by the ________ equation. (Q = K)
  • The equilibrium constant (K) is affected by ________ and ________ changes of precursors and products. (temperature, pressure)
  • The equilibrium constant (K) of a reaction can be determined experimentally by measuring the ________ of reactants and products at equilibrium. (concentrations)
  • The equilibrium constant (K) does not depend on the ________ of the reactants and products. (initial concentrations)
  • The equilibrium constant (K) indicates the reaction mixture at ________ equilibrium. (compound)
  • The equilibrium constant (K) can be used to predict the reaction ________. (direction)
  • The equilibrium constant (K) can be used to calculate the ________ of reactants or products at equilibrium if the concentration of other species is known. (unknown concentrations)
  • The equilibrium constant (K) is the temperature ________. (dependent)
  • The equilibrium constant (K) is usually used in the field ________. (chemical thermodynamics)
  • Le Chatelier’s principle states that when a system in equilibrium undergoes a change, it moves in such a way that ________ change restores equilibrium. (countermeasures)
  • Le Chatelier’s principle applies to ________ systems. (dynamic equilibrium)
  • According to Le Chatelier’s principle, an increase in pressure causes the equilibrium to change from ________ moles of gas. (fewer)

Chemical Equilibrium MCQs

Beyond the Navy, GD Pilots’ academic evaluations, Pakistan Air Force’s PAF Admin & Special Duty Branch, and PAF Aeronautical Engineering all value multiple choice questions on Chemical Equilibrium. The equilibrium concepts are thoroughly covered in these multiple-choice questions (MCQs), including the mathematical elements that are essential to passing these branches’ examinations.

Aspiring candidates can strengthen their knowledge of chemical equilibrium and perform better on the PAF’s academic examinations by studying these chemical equilibrium MCQs.

Chemical Equilibrium MCQ (Part-3)

  • Le Chatelier’s principle predicts that an increase in temperature causes an endothermic reaction to shift in the direction that ________ gets warmer. (absorbed)
  • Le Chatelier’s principle can be used to explain the effect of ________ on equilibrium. (concentration changes)
  • Le Chatelier’s principle states that the addition of ________ to a reaction mixture causes the equilibrium to shift in the direction that consumes the added substance. (reactive)
  • Le Chatelier’s principle can be used to explain the effect of ________ on the dissociation of a weak acid. (change in pH)
  • According to Le Chatelier’s principle, the removal of ________ from a reaction mixture causes the equilibrium to shift to produce more of the substance to be removed. (product)
  • Le Chatelier’s principle predicts that an increase in pressure will cause the volume of a system to ________. (decrease)
  • Le Chatelier’s principle can be used to explain the effect of ________ on salt solubility. (change in temperature)
  • According to Le Chatelier’s principle, an increase in the concentration of a reactant causes the equilibrium to move in a direction that ________ the concentration of the products. (increase)
  • Le Chatelier’s principle predicts that an exothermic reaction will shift to a warmer direction at ________ as the temperature decreases. (release)
  • According to Le Chatelier’s principle, the addition of ________ to a reaction mixture causes the equilibrium to move in a direction that decreases the added substance. (catalyst)
  • Le Chatelier’s principle can be used to explain the effect of ________ on the equilibrium position of a reversible reaction. (change in pressure)
  • According to Le Chatelier’s principle, an increase in temperature causes the equilibrium to shift in the direction that ________ heats up. (depletes)
  • According to Le Chatelier’s principle, an increase in temperature causes the equilibrium to shift to ________ warming. (absorbed)
  • Increasing the concentration of a reactant causes the equilibrium to shift to ________ the concentration of the products. (increase)
  • Addition of ____ to a reaction mixture can act as a catalyst and increase the rate of both forward and reverse reactions without affecting the equilibrium position. (catalyst)
  • Increasing the system pressure causes the equilibrium to shift to ________ moles of gas. (fewer)
  • A decrease in volume causes the equilibrium to shift in a direction that ________ the number of moles of gas. (reduce)
  • When ________ is added to a reaction mixture, it can react with the product and effectively remove it from the system, causing the equilibrium to shift toward the products. (reactive)
  • Raising the temperature of an exothermic reaction causes the equilibrium to shift in the direction that ________ heats up. (releases)
  • A decrease in temperature causes the equilibrium to shift to where ________ warms. (absorbed)
  • Increasing the concentration of a product causes a change in equilibrium, which ________ corresponds to the concentration of the reactants. (decrease)

Chemical Equilibrium Multiple Choice Questions(MCQ)

Chemical equilibrium multiple-choice questions(MCQ) are important not only for certain branches but also for the Technical Cadet Course, Army Education Officers, and Army EME Officers academic exams. These practice problems include mathematical elements and cover a wide range of equilibrium principles—a prerequisite for passing the Army’s examinations.

Through the use of chemical equilibrium these multiple-choice questions (MCQs), prospective candidates can strengthen their comprehension of equilibrium concepts and raise their scores on the Army’s academic tests.

Chemical Equilibrium MCQ (Part-4)

  • Addition of ____ to a reaction mixture can react with one reactant, effectively removing it from the system and causing the equilibrium to shift toward the reactants. (inhibitor)
  • Increasing the pressure in a system causes the volume of the system to ________. (decrease)
  • Increasing the temperature of an endothermic reaction causes the equilibrium to shift to ________ warming. (absorbed)
  • The decrease in pressure causes the equilibrium to shift to ________ moles of gas. (more)
  • Increasing the concentration of a reactant causes the equilibrium to move in a direction that ________ corresponds to the concentration of the reactants. (increase)
  • Addition of________ to a reaction mixture can react with a reactant or product, effectively consuming it and causing the equilibrium to shift toward the consumed substance. (consumption)
  • Solution equilibrium refers to the dynamic equilibrium between ________ and ________ of a solute in a solvent. (dissolution, precipitation)
  • The expression for the equilibrium constant of a soluble equilibrium is called the ________ multiplicative constant (Ksp). (solubility)
  • The solubility product constant (Ksp) is a measure of the ________ of a salt that is sparingly soluble in a solvent. (solubility)
  • The solubility product constant (Ksp) is equal to ________ of the ion concentrations in the equilibrium expression. (product)
  • The soluble product constant (Ksp) is temperature ________. (dependent)
  • The solubility of a salt is directly proportional to its solution product constant (Ksp) ________. (square root)
  • According to the general ion effect, the solubility of a salt decreases in the presence of the ________ ion, which is also a component of the salt. (common)
  • The solubility of most salts ________ with increasing temperature. (increase)
  • The solubility of a gas in a liquid ________ as the pressure increases. (increase)
  • The molar solubility of a salt is defined as the number of ________ salts that dissolve in one liter of solvent. (moles)
  • The solubility of a salt is affected by the ________ of the solvent. (polarity)
  • The solubility of a salt can be increased by ________ surface area of ​​the solid. (increases)
  • The solubility of a salt is affected by the amount of ________ in the solvent. (other solutes)
  • The solubility of a salt is often expressed in units of ________ per liter of solution. (in grams)
  • The solubility of a salt is often determined experimentally by constructing a ________ curve. (solubility)
  • An acid is a substance that gives ________ ions in a chemical reaction. (hydrogen)
  • A base is a substance that accepts ________ ions in a chemical reaction. (hydrogen)
  • The pH scale is a logarithmic scale that measures the ________ of a solution. (acidity)
  • A solution with a pH less than 7 is considered ________, while a solution with a pH greater than 7 is considered ________. (acidic, basic)
  • The dissociation of an acid in water produces ________ ions. (hydronium)
  • The dissociation of a base in water produces ________ ions. (hydroxide)
  • The strength of an acid or base is determined by its ________ ionization in water. (degree)
  • A strong acid ________ completely ionizes in water. (complete)
  • A weak acid ________ ionizes in water. (partially)
  • The dissociation constant (Ka) is a measure of the ________ of an acid in water. (strength)
  • pKa value is a logarithmic scale used to express the ________ of an acid. (acidity)

Important MCQs of Chemical Equilibrium MCQ with Answers

Important MCQs of Chemical Equilibrium MCQ with Answers are helpful not just for applicants hoping to enlist in the military but also for citizens getting ready for military exams. These practice problems provide a solid comprehension of the subject matter by covering a wide range of equilibrium principles.

Candidates can become more proficient in chemical equilibrium and perform better on tests administered by the armed forces by working through these chemical equilibrium multiple-choice questions.

Chemical Equilibrium MCQ (Part-5)

  • A neutralization reaction involves a reaction between an acid and a base, resulting in ________ and a salt. (water)
  • The Henderson-Hasselbalch equation relates the ________ of an acid or base to its pKa value and the ratio of conjugate base to acid. (pH)
  • An indicator is a substance that changes ________ according to the pH of a solution. (color)
  • The buffer volume of a phrase indicates its ability ________ to change pH. (resist)
  • In industrial processes, equilibrium is often achieved by ________ reactions. (reversible)
  • Haber’s process is used for the synthesis of ________. (ammonia)
  • The equilibrium constant (K) of a reaction can be used to predict the reaction at ________ equilibrium. (range)
  • Increasing the pressure in a system at equilibrium can move the equilibrium to ________ moles of gas. (less)
  • The queuing process is used in the production of ________. (sulfuric acid)
  • The equilibrium constant (K) of the reaction is not affected by changes in ________ conditions. (concentration)
  • The temperature at which a reaction reaches equilibrium is called the ________ temperature. (equilibrium)
  • The expression for the equilibrium constant (K) of a reaction is determined by the equation ________. (equilibrated)
  • A change in equilibrium caused by a change in concentration of a reactant or product is described by the ________ principle. (Le Chatelier’s)
  • Raising the temperature during an exothermic reaction causes the equilibrium to shift to ________ heat. (absorbed)
  • Making ethanol by fermentation is an example of a ________ process. (biochemical)
  • The equilibrium constant (K) of a reaction can be changed by changing the ________ of the reaction. (temperature)
  • The change in equilibrium caused by a change in system pressure is described by the ________ principle. (Le Chatelier)
  • The equilibrium constant (K) of a reaction is the ratio of the concentrations of the products ________ to the concentrations of the reactants. (concentrations)
  • The change in equilibrium caused by a change in the temperature of a system is described by the ________ principle. (Le Chatelier’s)

See More

  • Initial Tests of Chemistry for Pak Navy Tests (Download)
  • Past Experience of Chemistry MCQs for Pak Navy Sailors Tests (Download)
  • Free Online Practice of Past Experiences for Chemistry Tests (Download)
  • Free Practice of Past Papers of Advance Chemistry Questions (Download)

Join us at Social Media

More MCQs of Past Experiences to Join Pak Forces

Similar Posts