Tag: adsorption and colloids

Quizzes (5) Questions (127)

Questions Related to adsorption and colloids

Multiple choice enzymes and catalysts catalysis adsorption and colloids surface chemistry chemistry adsorption theory of heterogeneous catalysis

A catalyst:

  1. changes $\Delta G$ for an equation

  2. acts by increasing the rate of the forward reaction more than the reverse reaction

  3. raises the equilibrium constant of a system
  4. may have a molecular weight as low as $1$ or higher than $200,000$
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Gibbs free energy change is a state function which does not depend upon the path taken by the reaction whereas catalyst change path by lowering activation energy.

Catalysts increase the rate of the reaction but have no effect on the yield and catalysts speed up both forward and reverse reaction hence it doesn't change equilibrium constant.

Catalyst doesn't need to be so bulky otherwise instead of fastening the reactions it decreases the speed of reaction. But its weight can be as low as 1 or as high as 200000.

Multiple choice enzymes and catalysts catalysis adsorption and colloids surface chemistry chemistry adsorption theory of heterogeneous catalysis

What can cause a decrease in activation energy?

  1. An increase in the reactant concentration

  2. An increase in the temperature

  3. A decrease in pressure

  4. Catalysts
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Option D is the correct answer.

Catalysts decrease the activation energy required for a chemical reaction and increase the rate of the reaction.

Multiple choice enzymes and catalysts catalysis adsorption and colloids surface chemistry chemistry adsorption theory of heterogeneous catalysis

Statement $1$: A catalyst increases the equilibrium of a reaction.
Statement $2$: Catalysts only lower the activation energy of the forward reaction.

  1. Both Statement $1$ and Statement $2$ are correct and Statement 2 is the correct explanation of Statement $1$
  2. Both Statement $1$ and Statement $2$ are correct, but Statement $2$ is NOT the correct explanation of Statement $1$
  3. Statement $1$ is correct, but Statement $2$ is not correct
  4. Both the Statement $1$ and Statement $2$ are not correct
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Catalysts work by producing an alternative route for the reaction. This affects the forward and back reactions equally so there is not any change in equilibrium.

Further catalysts speed up both forward and reverse reactions otherwise its equilibrium constant get change which further change the equilibrium

Multiple choice enzymes and catalysts catalysis adsorption and colloids surface chemistry chemistry adsorption theory of heterogeneous catalysis

Which of the following statement(s) is/are $NOT$ correct regarding chemical catalysts?

  1. They are not consumed during the chemical reaction.

  2. They cannot make non-spontaneous reactions occur.

  3. They do not have to be the same phase as the reactant molecules.

  4. They shift equilibrated reactions to the product's side.
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Catalyst only alters the pathway of reaction by lowering the activation energy. They don't use in any reaction and remain unconsumed after the reaction.

Since they are lowering the activation energy so reactants easily cross the barriers and make no-spontaneous reactions occur

It is not necessary that catalysts are in the same phase with reactants such catalysis called heterogeneous catalysis.
For eg. $2SO _2(g) \xrightarrow{Pt(s)} 2SO _3(g)$

The equilibrium constant does not change in reaction by the catalyst which means that equilibrium doesn't shift in any direction. Hence option D is not correct.

Multiple choice enzymes and catalysts catalysis adsorption and colloids surface chemistry chemistry adsorption theory of heterogeneous catalysis

A catalyst:

  1. increases the free energy change in the reaction

  2. decreases the free energy change in the reaction

  3. does not increase or decrease the free energy change in the reaction

  4. can either decrease or increase the free energy change depending on what catalyst we use
Reveal answer Fill a bubble to check yourself
C Correct answer
Explanation

A catalyst is a substance which increases the free energy change(rate of reaction) in the reaction.But is not consumed by the reaction; hence a catalyst can be recovered chemically unchanged at the end of the reaction it has been used to speed up or catalyze.

Multiple choice enzymes and catalysts catalysis adsorption and colloids surface chemistry chemistry adsorption theory of heterogeneous catalysis

Which of the following statements is more correct?

  1. A catalyst only accelerates the rate of a chemical reaction.

  2. A catalyst can retard the rate of a chemical reaction.

  3. A catalyst can control the speed of a reaction.

  4. A catalyst alters the speed of a reaction.
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

A catalyst is a substance which increases (accelerate)  the rate of reaction.But is not consumed by the reaction; hence a catalyst can be recovered chemically unchanged at the end of the reaction it has been used to speed up, or catalyze. 

Multiple choice enzymes and catalysts catalysis adsorption and colloids surface chemistry chemistry adsorption theory of heterogeneous catalysis

Which of the following statements is not true?

  1. The action of a catalyst is not specific.

  2. The catalyst does not alter the equilibrium.

  3. A small amount of catalyst is sufficient to catalyse large amounts of reactants.

  4. The catalyst initiates the reaction.
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation

All catalysts are specific for certain  reactants. A certain catalyst can react with a particular reactant only. All catalysts do not react with all reactants.
Hence option A is correct.

Multiple choice enzymes and catalysts catalysis adsorption and colloids surface chemistry chemistry adsorption theory of heterogeneous catalysis

Edges and peaks are more effective in a catalyst because: 

  1. they have more free valencies

  2. they have limited number of atoms

  3. they have limited number of molecules

  4. none of the above
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation

Edges and peaks of catalyst are the interacting sites of catalysts with the reagents as they have free valencies.So edges and peaks are effective sites of catalysts.
Hence option A is correct

Multiple choice enzymes and catalysts catalysis adsorption and colloids surface chemistry chemistry adsorption theory of heterogeneous catalysis

The substance which decreases the rate of a chemical reaction is called: 

  1. inhibitor

  2. poison

  3. moderator

  4. promoter
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation

The substance which decreases the rate of a chemical reaction is called inhibitor e.g. anti-oxidants are added as inhibitors to food substances to stop its spoilage from exposure oxygen. Similarly, protective coatings on metal surfaces inhibit the corrosion of metals by preventing their interaction with the air and water. An inhibitor is an opposite of a catalyst.

Multiple choice enzymes and catalysts catalysis adsorption and colloids surface chemistry chemistry adsorption theory of heterogeneous catalysis

In the reaction, $KMnO _4 + H _2SO _4 + H _2C _2O _4\xrightarrow{Mn^{2+}}$ Products, $Mn^{2+}$ ions act as:

  1. positive catalyst

  2. negative catalyst

  3. autocatalyst

  4. enzyme catalyst
Reveal answer Fill a bubble to check yourself
C Correct answer
Explanation

Purple permanganate ions are reduced in acidic solution by oxalate ions to the nearly colorless manganese(II) ions, whereas the oxalate ions are oxidized to gaseous carbon dioxide: Obviously, the $Mn^{2+}$  ions act as catalyst. The reaction rate increases gradually even when no $Mn^{2+}$ ions are added because they are formed during the reaction meaning this product autocalyzes its own formation.