Homogeneous Equilibrium MCQ Quiz - Objective Question with Answer for Homogeneous Equilibrium - Download Free PDF

The Correct answer is it exhibits uniform composition throughout.

Key Points

• An alloy is a mixture of two or more metals, or a metal and a non-metal.
• It is considered a homogeneous mixture because it has a uniform composition throughout.
• This means that the properties and composition of the alloy are the same in every part of the material.
• Examples of alloys include brass (copper and zinc), steel (iron and carbon), and bronze (copper and tin).
• Alloys are used in various applications such as construction, automotive, aerospace, and electronics industries due to their enhanced properties.
• The ability to combine different elements allows alloys to have improved strength, durability, and resistance to corrosion compared to pure metals.

 Additional Information

•  contains two or more phases
  • A material with two or more phases is a heterogeneous mixture, not homogeneous.
  • In a heterogeneous mixture, different components can be observed separately.
• its components can be separated by filtration
  • Filtration is a method used to separate solid particles from liquids or gases, generally applicable to heterogeneous mixtures.
  • Alloys do not separate into their components through simple physical methods like filtration.
• its components are chemically combined in fixed proportions
  • While alloys are mixtures, not compounds, their components are combined in variable, not fixed, proportions.
  • Compounds have a fixed ratio of elements, whereas alloys can vary in composition to achieve desired properties.

The correct answer is Carbon dioxide and water.

Key Points

• Carbon dioxide (CO₂) and water form a homogeneous mixture when CO₂ dissolves uniformly in water under standard conditions.
• This mixture is seen in carbonated beverages where CO₂ is dissolved in water to create a fizzy effect.
• The solubility of CO₂ in water is enhanced under higher pressure and lower temperatures.
• The dissolution of CO₂ in water produces a weak acid known as carbonic acid (H₂CO₃), contributing to the homogeneous nature of the solution.
• Homogeneous mixtures are characterized by a single-phase appearance where the components are evenly distributed.

Additional Information

• Homogeneous Mixture
  • A homogeneous mixture is a mixture where the components are evenly distributed at the molecular level, resulting in a uniform composition.
  • Examples include solutions such as sugar dissolved in water, saltwater, and air.
• Heterogeneous Mixture
  • In a heterogeneous mixture, the components remain distinct and can often be visually differentiated.
  • Examples include sand and water, oil and water, and soil mixtures.
• Solubility of Gases in Liquids
  • The solubility of gases in liquids depends on factors like pressure, temperature, and the nature of the gas and liquid.
  • Higher pressure increases gas solubility, as seen in carbonated drinks where CO₂ is dissolved under pressure.
• Carbonic Acid (H₂CO₃)
  • When CO₂ dissolves in water, it reacts to form carbonic acid, which is a weak acid.
  • This reaction is reversible and plays a role in regulating the pH of natural water bodies and blood in living organisms.

The correct answer is Oil in water.

Key Points

• A homogenous mixture is a mixture that has the same uniform appearance and composition throughout.
• Examples of homogenous mixtures include solutions such as salt dissolved in water, sugar dissolved in water, and copper sulphate powder in water.
• Oil in water is not a homogenous mixture because oil and water do not mix evenly and form separate layers, making it a heterogeneous mixture.
• In a heterogeneous mixture, the components are not uniformly distributed and can often be easily separated.
• Homogenous mixtures have a single phase, whereas heterogeneous mixtures have two or more phases.

Additional Information

• Solutions
  • These are homogenous mixtures where one substance (the solute) is dissolved in another substance (the solvent).
  • Common examples include salt water and sugar water.
• Suspensions
  • These are heterogeneous mixtures where solid particles do not dissolve but are suspended in a liquid or gas.
  • Examples include sand in water or flour in water.
• Colloids
  • These are mixtures where very small particles of one substance are evenly dispersed throughout another substance.
  • Examples include milk, mayonnaise, and gelatin.

The correct answer is Orange juice with pulp.

Key Points

• A homogeneous mixture is one that has a uniform composition and appearance throughout.
• Orange juice with pulp is a heterogeneous mixture because the pulp is not uniformly distributed throughout the liquid.
• In a heterogeneous mixture, the different components are visibly distinguishable.
• Other examples provided, such as pure air, sugar solution, and vinegar, are homogeneous mixtures where components are evenly distributed.

Additional Information

• Homogeneous Mixture
  • A mixture in which the composition is uniform throughout the mixture.
  • Examples: Salt water, air, and vinegar.
  • These mixtures have the same phase and properties throughout.
• Heterogeneous Mixture
  • A mixture in which the composition is not uniform throughout the mixture.
  • Examples: Salad, sand and water, and orange juice with pulp.
  • Different phases and properties can be observed in different parts of the mixture.
• Solution
  • A type of homogeneous mixture composed of two or more substances.
  • The solute is the substance that is dissolved, and the solvent is the substance that does the dissolving.
  • Examples: Sugar in water, salt in water.
• Colloid
  • A mixture where very small particles of one substance are evenly distributed throughout another substance.
  • Examples: Milk, mayonnaise, and jelly.
  • Particles do not settle and cannot be separated out by ordinary filtering or centrifuging like those in a suspension.

The correct answer is Oil in water.

Key Points

• A homogenous mixture is a mixture that has the same uniform appearance and composition throughout.
• Examples of homogenous mixtures include solutions such as salt dissolved in water, sugar dissolved in water, and copper sulphate powder in water.
• Oil in water is not a homogenous mixture because oil and water do not mix evenly and form separate layers, making it a heterogeneous mixture.
• In a heterogeneous mixture, the components are not uniformly distributed and can often be easily separated.
• Homogenous mixtures have a single phase, whereas heterogeneous mixtures have two or more phases.

Additional Information

• Solutions
  • These are homogenous mixtures where one substance (the solute) is dissolved in another substance (the solvent).
  • Common examples include salt water and sugar water.
• Suspensions
  • These are heterogeneous mixtures where solid particles do not dissolve but are suspended in a liquid or gas.
  • Examples include sand in water or flour in water.
• Colloids
  • These are mixtures where very small particles of one substance are evenly dispersed throughout another substance.
  • Examples include milk, mayonnaise, and gelatin.

Key Points

Mixture-

• A mixture is described as a result of combining two or more substances.
• Each substance maintains its chemical identity.
• In other words, within the components of a mixture, a chemical reaction does not occur. 

• Homogeneous mixture:
  • A homogeneous mixture is a liquid, gaseous & solid mixture.
  • Throughout any given sample, it has the same proportions of its components 
  • The mixture has the composition throughout & the same uniform appearance in every step
  • Many homogeneous mixtures are generally referred to as solutions.
• Example:
  • Some examples of homogeneous mixtures:
    including air, mixture, saline solution, most alloys, bitumen, blood plasma, etc.​

​Mistake Points

• The question asks about 'blood plasma' and not 'blood', which are not the same.
• Blood plasma is a light yellowish liquid that forms about 55% of blood.
• Blood comprises blood plasma and the blood cells like RBCs, WBCs, etc.
• Therefore, blood plasma is a homogeneous mixture, while blood is a heterogeneous mixture.

The correct answer is Colloids are homogeneous mixtures.

Key Points

Concept:

Colloidal solution/ colloid:

• The type of solution in which the size of the solute particle is in the range of 1 to 100 nm, is called a colloid.
• A colloid is a heterogeneous system in which one substance is dispersed (dispersed phase or colloidal particles) in another substance which is called a dispersion medium.

Explanation:

Properties of colloids:

• A colloid appears to be homogeneous but actually, it is heterogeneous.
• The particles of most of the colloids cannot be seen even with a microscope.
• It scatters a beam of light passing through it (Tyndall effect).
• The size of the solute particle is in the range of 1 to 100 nm.
• Since they are heterogeneous in nature, centrifugation techniques can be used to separate the particles.

Additional Information

The correct answer is Both I and II.

• Both statements regarding the use of bleaching powder are correct.

Key Points

• Bleaching powder is a pale yellowish powder existing with a strong smell of chlorine.
• It is soluble in water but due to the presence of impurities, we never observe a clear solution.
• Its chemical formula is Ca(OCl₂) with its chemical name as Calcium hypochlorite.
• Bleaching powder (CaOCl₂ ​) has many uses and some of them are as follows:
  • It is used in bleaching dirty clothes in launder, as a bleaching agent in cotton and linen in the textile industry.
  • Due to the evolution of nascent oxygen.
  • It is used as an oxidizing agent in the chemical industries.
  • It can be used as a disinfectant which can be used for disinfecting water to make it potable.

The correct answer is Physical properties.

Key Points

• The physical properties help in separating the homogenous mixtures.
• Those mixtures in which the substances are completely mixed together and are indistinguishable from one another are called homogeneous mixtures.
• A homogeneous mixture is a mixture in which the composition is uniform throughout the mixture.
• Some of the examples of homogeneous mixtures (or solutions) are Sugar solution, Salt solution, Copper sulphate solution, Seawater, Alcohol and water mixture, Petrol and oil mixture, Soda water etc.

Explanation:

•  Mixture: When two or more substances mix with each other without taking part in a chemical change, the resulting substance is called a Mixture. For example seawater, crude oil, Ink, air etc.
• The mixer is two types: homogeneous mixer and heterogeneous mixer.

• The properties of the mixtures may or may not be the same as those of its components depending upon the type of the mixture. A mixture is formed as a result of physical change only.

So, air is a mixture.

• When two or more substances mix in fix ratio with each other after taking part in a chemical change, the resulting substance is called a compound.
• Their physical and chemical properties are the same at every molecule. For example water, CO₂ etc.

Mistake Points

• A colloidal solution in which liquid particles are dispersed in a liquid medium is known as an emulsion.
• Milk is an emulsion in which fat globules are suspended in water. 

The correct answer is Colloidal solution is homogenous in nature.

Key Points

• The particles in colloidal solutions are uniformly distributed at the molecular level. Hence statement 1 is correct.
  • Colloidal particles are dispersed and their distribution is uneven.
  • Particles are larger than individual molecules but smaller than the molecules in suspension.
  • The colloidal state is characterized by the presence of finely divided particles that remain dispersed and are not stable.
• The term "colloid" refers to a system where one substance is finely dispersed in another.
• Colloidal solutions are heterogeneous at the microscopic level due to the presence of dispersed particles. Hence statement 2 is not correct.
  • The particles are small enough to remain dispersed and not settle out, resulting in a stable colloidal solution that has a uniform appearance.
• Tyndall effect is the scattering of light by colloidal particles. Hence statement 3 is correct.
  • When a beam of light passes through a colloidal solution, the scattered particles scatter the light, making the path of the beam visible.
  • This effect is not seen in real solutions, where the particles are small and do not scatter light significantly.
• Colloidal particles are small enough to experience Brownian motion, which prevents them from settling under the influence of gravity.
  • This is a distinctive feature of colloids, and it contributes to their stability. Hence statement 4 is correct.

The correct answer is Only III. 

Key Points

• The particles of a suspension can be seen by the naked eyes.
• Solute particles settle down when left undisturbed.
• Larger particles in a suspension can be separated from the liquid or air by filtration.
• Suspension is a heterogeneous mixture. 

Additional Information 

• Suspension: A suspension is a heterogeneous solution in which, while standing, several particles move out of the mixture.
  • In a suspension, the volume of the solvent particles is quite high. It has a length of more than 100 mm.
  • It is easy to see the molecules of a suspension.
  • A suspension’s particles don’t go through a filter paper. Thus, filtration can separate a suspension.
  • There’s shaky suspension. After some time a suspension’s particles settle down.
  • Due to its large particle size, a suspension disperses a light beam that passes through it.
• Heterogeneous mixture: This is a type of mixture in which all the components are completely mixed and all the particles can be seen under a microscope.
• Key points regarding this type of mixture:
  • Particles are distributed non-uniformly.
  • We can judge a heterogeneous mixture by just seeing it.
  • Non-uniform composition.
  • Example: seawater, pizza, etc.
• Homogenous mixture: These are the types of mixtures in which the components mixed are uniformly distributed throughout the mixture.
• Key points regarding such mixtures are:
  • Particles are distributed uniformly.
  • We can’t judge a homogeneous mixture by just seeing it.
  • Homogeneous mixtures are also called solutions.
  • Uniform composition.
  • Example: rainwater, vinegar, etc.

Explanation:

Le- Chatelier's principle:

• Equilibrium is a condition that occurs when a chemical reaction is reversible, and the forward and reverse reactions occur simultaneously, at the same rate.
• Le Chatelier's Principle- "if a chemical system at equilibrium experiences a change in concentration, temperature or total pressure, the equilibrium will shift in order to minimize that change".
• ​Effect of change of concentration:
  • According to Le - Chatelier's Principle, when the concentration of one of the reactants in a system at equilibrium is increased so that the system is no longer at equilibrium, instantaneously, then the equilibrium will shift so as to decrease the concentration of the reactant.
  • This means the equation or equilibrium will shift forward.
  • If there is an increase in the concentration of any of the products, then the equilibrium shifts towards the backward direction so as to decrease the concentration of the products.
• Effect of change of pressure:
  • Change of pressure will have no effect on the state of equilibrium if;
  • The system does not involve gaseous reactants or products.
  • The number of moles of gaseous reactants and products is equal on both sides.
  • According to Le- Chatelier's principle, on increasing the pressure, the rate of reaction will shift to the side where there is a decrease of pressure or a lesser number of moles of gaseous components.
• Effect of addition of inert gas:
  • When an inert gas is added to an equilibrium system at constant volume, there will be an increase in the total pressure of the system. The concentrations of the products and reactants will not change. There will be no change in the position of the equilibrium.
  • This is because the ratio of the moles of the components to the volume of the container will not change.
  • When a gas is added to the system at equilibrium keeping the pressure constant, the volume increases.
  • This causes a decrease in the number of moles of gases per unit volume.
  • Hence, the equilibrium shifts towards the direction in which there is an increase in the number of moles of gases.

Hence,  when an inert gas is added to the system at equilibrium but pressure remains unchanged, It remains unaffected

Additional Information

• When a catalyst is introduced at equilibrium, there will be no change in the rate of the reaction.

Concept:

Haber's process:

• This process is used in large scale preparations of ammonia.

N2 + 3H2 → 2NH3

• During the process, nitrogen and hydrogen are used in the ratio 1:3.
• The process is exothermic ΔH = -ve  in nature means heat is produced in the process.
• According to the Le-chateliar principle, the temperature is kept high to speed up the process.
• The gaseous ammonia produced is converted to liquid ammonia to remove the products formed.
• This drives the reaction forward.

Equilibrium Constants:

• ​The constants K_p and K_c are both equilibrium constants.
• K_p is used when the concentration terms are given in partial pressures i.e, in gaseous reactions.
• K_c is used when the reaction terms are expressed in molarities.
• The relation between K_p and K_c is given by:

\({K_p} = {K_c} \times {\left( {RT} \right)^{\Delta n}}\) where R = Universal gas constant, T = Temperature, and \(\triangle n\) = change in moles of gases in the reaction.

Calculation:

• ​The relation between K_p and K_c is

\({K_p} = {K_c} \times {\left( {RT} \right)^{\Delta n}}\)

For the reaction

N2(g) + 3H2(g) \(\rightleftharpoons\) 2NH3(g)

\(No.\;of\;moles\;of\;products = 2\)

\(No.\;of\;moles\;of\;reactants = 3 + 1 = 4\)

\(Change\;in\;number\;of\;moles\;of\;gases = {n_{products}} - {n_{reactants}} = \;\Delta n\)

\( = 2 - 4 = - 2\)

Hence,

\({K_p} = {K_c} \times {\left( {RT} \right)^{-2}}\)

Hence, or the reaction N2(g) + 3H2(g) \(\rightleftharpoons\) 2NH3(g) ΔH = -ve, \({K_p} = {K_c} \times {\left( {RT} \right)^{-2}}\)

Explanation:

The correct option is Small difference (less than 25° C) in their boiling points

Fractional distillation:

• Fractional distillation is the separation of a mixture into its component parts or fractions. Chemical compounds are separated by heating them to a temperature at which one or more fractions of the mixture will vaporize. It uses distillation to fractionate.
• Generally, the component parts have boiling points that differ by less than 25 °C (45 °F) from each other under the pressure of one atmosphere. 
• The method of distillation is used to separate the liquids having sufficient differences in their boiling points. Liquids having different boiling points vaporise at different temperatures, the vapours are cooled and the liquids so formed are collected separately. 
• The technique of fractional distillation is used in such cases where vapours of a liquid mixture are passed through a fractionating column before condensation. The fractionating column is fitted over the mouth of the round bottom flask.
• Vapours of the liquid with a higher boiling point condense before the vapours of the liquid with a lower boiling point. By the time the vapours reach the top of the fractionating column, these are rich in the more volatile component.
• A fractionating column provides many surfaces for heat exchange between the ascending vapours and the descending condensed liquid.
• One of the technological applications of fractional distillation is to separate different fractions of crude oil in the petroleum industry.

Additional Information

• Simple distillation- It is a procedure by which two liquids with different boiling points can be separated. Large difference (greater than 25° C) in the boiling points of liquid

• A vacuum distillation is used when the boiling point of the compound is too high (Tb>150oC) in order to distil the compound without significant decomposition.