CBT TEST Fuoye

CHM 203 CBT PRACTICE TEST

Ace/Undergragra January 20, 2024

2 3,426 1 minute read

Take your time to read instructions before taking this test.

There are 40 questions which you are to answer in 15 minutes that gives you roughly 30 seconds per question.

If you can get at least 60%, you can be rest assured that you’ll ace CHM 203 exam

In a normal exam you will be asked between 40 – 60 questions but I only arranged 40 questions

Note

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Move as fast as possible and starting with questions that don’t have calculation first to save time

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70 – 100 A

60 – 69 B

50 – 59 C

45 – 49 D

40 – 44 E

0 – 39 F

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CHM 203

1 / 39

All of the following processes lead to an increase in entropy EXCEPT

A. forming mixtures from pure substances.

B. evaporating a liquid.

C. increasing the temperature of a gas.

D. freezing a liquid.

2 / 39

Which of these followings would lead to an increase in the internal energy of a system?

A. Work done by the system

B. Work done on the system

C. Loss of heat from the system

D. Adiabatic expansion of the system

3 / 39

Thermodynamics can be used to determine all of the following EXCEPT

A. the extent to which a reaction occurs.

B. the temperature at which a reaction is spontaneous.

C. the rate of reaction.

D. the direction in which a reaction is spontaneous

4 / 39

Which of these is true of an isochoric system?

A. Pressure is not constant

B. Heat is allowed into the system but not allowed out of the system

C. Takes place at constant temperature

D. Volume remains constant

5 / 39

Milk sours more rapidly in summer than in winter because

A. None of the options

B. in summer, the energy of activation decreases and hence the of reaction becomes fast

C. in winter, number of molecules per unit volume increases and hence the rate of reaction becomes fast

D. in summer, the temperature Is high due to which effective collisions increase and hence the rate of reaction becomes fast

6 / 39

The first law of thermodynamics deals with

A. thermodynamic equivalence

B. Entropy

C. conservation of energy

D. absolute zero temperature.

7 / 39

One mole of an ideal gas is heated at a constant pressure of 101300 N $m^{2}$, from 273.2 K to 373 K. Calculate the work involved R = 8.314 J/mol/K).

A. 8.314 J/mol

B. 83.14 J/mol

C. 8314 J/mol

D. 831.4 J/mol

8 / 39

A beaker with a mixture of ice and water is maintained at equilibrium: H2O(s) + heat➡️H2O(l); If the temperature of the system is decreased:

A. Water freezes to form ice (shifts to the left)

B. Ice melts to form liquid water (shift to the right)

C. No change occurs

D. The container cacks

9 / 39

Powdered marble reacts more rapidly with HCl than the chips of marble because:

A. Marble chips will not react with HCl

B. Surface area of powdered marble is more that of chips of marble and hence there is more collisions between the molecules of reactants

C. Energy of activation decreases

D. Number of molecules increases.

10 / 39

10.

In the reaction: 2B ➡️Product; the rate equation is: Rate = k[B]. If the concentration of is doubled, the rate of reaction will increase by a multiple of

A. 3

B. 4

C. None

D. 2

11 / 39

11.

The reactions with the high value of energy of activation are

A. Fast

B. Slow

C. Moderate

D. Not feasible

12 / 39

12.

Of the following product-favoured processes, which are endothermic? 1. the combustion of methane to produce water and carbon dioxide. 2. the expansion of an ideal gas. 3. the melting of ice at temperatures greater than 0ºC.

A. 2 and 3

B. 3

C. 1

D. 2

13 / 39

13.

If the reaction A + B C has an equilibrium constant greater than one, which of the following statements is correct?

A. The backward rate of reaction is slow.

B. The forward rate of reaction is fast.

C. The reaction is product favoured.

D. The reaction is not spontaneous

14 / 39

14.

A reaction with a negative value of 🔼G is said to be

A. At equilibrium

B. Non-spontaneous

C. Spontaneous

D. Reversible

15 / 39

15.

Which of the following expressions is associated with the law of conservation of energy?

A. dE = q + w

B. dG = dH TdS

C. q = mCdT

D. H = E + PV

16 / 39

16.

The specific heat of silver is 0.0565 $cal/g/^{o}C$. Assuming no loss of heat to the surroundings or to the container, calculate the final temperature when 100 g of silver at 40 $^{o}C$ is immersed in 60 g of water at 10 $^{o}C$.

A. 16.2 $^oC$

B. 21.6 $^oC$

C. 25 $^oC$

D. 12.6 $^o C$

17 / 39

17.

The reactions catalyzed by sunlight are called ____________ reactions

A. photochemical

B. Endothermic

C. Exothermic

D. Sun-lighted

18 / 39

18.

Which of the following involves a decrease in entropy?

A. the dissolution of NaCl in water

B. the sublimation of carbon dioxide

C. the freezing of liquid water into ice

D. . the evaporation of ethanol

19 / 39

19.

Every type of chemical bond contains a certain amount of energy. The total bond energy, which is essentially equivalent to the total potential energy of the system, is a quantity known as:

A. kinetic energy.

B. entropy

C. free energy.

D. enthalpy.

20 / 39

20.

If a chemical reaction has a positive change in entropy, 🔼S, then

A. the Gibbs free energy is negative

B. heat goes from the system into the surroundings

C. . the disorder of the system increases

D. the reaction is exothermic.

21 / 39

21.

In a reaction: 2A ➡️B + 2C, which of the statement is true?

A. Rate of disappearance of A = Rate of formation of B

B. Rate of formation of C= Rate of formation of B

C. Rate of formation of B = Rate of disappearance of A

D. Rate of disappearance of A = Rate of formation of C

22 / 39

22.

A statement of the second law of thermodynamics is that

A. spontaneous reactions are always exothermic.

B. the enthalpy of reaction is the difference between product and reactant enthalpies.

C. energy is conserved in a chemical reaction.

D. the entropy of the universe is continually increasing

23 / 39

23.

Table of Contents

Which of the following statements about enthalpy is incorrect?

A. Reactions which absorb heat have a positive DH

B. enthalpy is a state function

C. $Delta H$ is the enthalpy change at constant pressure

D. Enthalpy and internal energy of a system are always identical

24 / 39

24.

The heat of combustion for 1 mole of carbon to carbon dioxide is -410 kJ. How many kJ of heat would be liberated from the complete combustion of 60.0 g of carbon?

A. -24,600 kJ

B. 650.2 kJ

C. -2050 kJ

D. A. -82 kJ

25 / 39

25.

All of the following statements concerning entropy are true EXCEPT

A. entropy values are greater than or equal to zero.

B. entropy is a state function.

C. . entropy is zero for elements under standard conditions.

D. a positive change in entropy denotes a change toward greater disorder

26 / 39

26.

Which of the following statements about the kinetics of the reaction H2(g) + Br2(g) ➡️2HBr(g) is definitely true?

A. The reaction is second order overall.

B. The presence of hydrogen bromide, HBr, inhibits the rate of the reaction

C. The reaction is first order with respect to bromine, Br2.

D. It is not possible to determine anything about the kinetics of the reaction from the stoichiometry

27 / 39

27.

When extra NH3 is added to the following system at equilibrium: 3H2(g) + N2(g) ➡️ 2 NH3(g), what happens?

A. Concentration of hydrogen decreases, but that of hydrogen increases

B. In order to restore equilibrium, the reaction shifts right, toward product

C. No change occurs

D. In order to restore equilibrium, the reaction shifts left, toward reactants

28 / 39

28.

Calculate the standard entropy change for the following reaction, 2Ag2O(s) ➡️4 Ag(s) + O2(g); given S^{o}[Ag2O] = 121.3 J/K·mol, S^{o}[Ag(s)] = 42.6 J/K·mol, and S^{o}[O2(g)] = 205.1 J/K·mol.

A. + 132.9 J/K2

B. + 126.4 J/K

C. -126.4 J/K

D. -205.1 J/K

29 / 39

29.

Which reaction is likely to have a negative change in entropy?

A. 2NH3(s) ➡️N2(g) + 3 H2(g)

B. NaCl(s) ➡️Na^+(aq) + Cl^-(aq)

C. CaO(s) + CO2(g) ➡️ CaCO3(s)

D. N2O4(g)➡️2 NO2(g)

30 / 39

30.

The minimum additional energy, above the average internal energy, which the reacting molecules must possess so that their collision result in a reaction is known as

A. Threshold Energy

B. Kinetic Energy

C. Thermodynamic Energy

D. Activation Energy

31 / 39

31.

The temperature remains constant as energy is added to a substance. How may the substance be changing?

A. From a liquid to a gas

B. From a gas to a solid

C. From a liquid to a solid

D. Change in the amoung of kinetic energy

32 / 39

32.

In a reaction in which the rate of the reverse reaction is equal to the rate of the forward reaction, a state of ____________ is attained.

A. dynamic equilibrium

B. thermodynamics

C. product reversibility

D. total entropy

33 / 39

33.

Rusting of iron Is an example of________ reaction

A. Fast

B. Moderate

C. Explosive

D. Slow

34 / 39

34.

Calculate the standard entropy change for the following reaction, 2 Ag2O(s) ➡️4 Ag(s) + O2(g)

given S^{o}[Ag2O] = 121.3 J/K·mol, S^{o}[Ag(s)] = 42.6 J/K·mol, and S^{o}[O2(g)] = 205.1 J/K·mol.

A. -205.1 J/K

B. +132.9 J/K2

C. +126.4 J/K

D. -126.4 J/K

35 / 39

35.

For a reaction: 2H2+ 2NO ➡️2H2O + N2 the rate law is R = K [H2][NO]^2 The Order of the reaction is?

A. 1

B. 3

C. 0

D. 2

36 / 39

36.

Predict the signs of 🔼H and 🔼S for the evaporation of water at 35 ^oC.

A. 🔼 H 0

B. 🔼 H > 0 and 🔼S < 0

C. 🔼H > 0 and 🔼S > 0

D. 🔼H < 0 and 🔼S < 0

37 / 39

37.

If a gas absorbs 1000 J of heat and expands by 0.5 $dm^{3}$ against a constant pressure of 4 atms (1 atm = 100000 Pa), then the change in internal energy is approximately

A. -1200 J

B. -800 J

C. 800 J

D. 1200 J

38 / 39

38.

The common-ion effect

A. promotes condensation

B. increases solubility

C. promotes evaporation

D. reduces ionization.

39 / 39

39.

If a process is exothermic and not spontaneous, then what must be true?

A. 🔼S > 0

B. 🔼 G = 0

C. 🔼 S < 0

D. 🔼H > 0$

Your score is

The average score is 31%

Ace/Undergragra January 20, 2024

2 3,426 1 minute read

2.5 2 votes

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Mercy

5 months ago

Pls how about for AEB

Author

Reply to Mercy

What’s the course code ?

Blessing
Please sir,can we get Bus 106 & 102¿...
Blessing
Can we get more questions please?...
Blessing
Please can you drop IRP CBT?...
Ace/Undergragra
When do you have it and can you text me on Whatsapp please?...
Emmanuel
Irp 102...

All of the following processes lead to an increase in entropy EXCEPT

Which of these followings would lead to an increase in the internal energy of a system?

Thermodynamics can be used to determine all of the following EXCEPT

Which of these is true of an isochoric system?

Milk sours more rapidly in summer than in winter because

The first law of thermodynamics deals with

One mole of an ideal gas is heated at a constant pressure of 101300 N $m^{2}$, from 273.2 K to 373 K. Calculate the work involved R = 8.314 J/mol/K).

A beaker with a mixture of ice and water is maintained at equilibrium: H2O(s) + heat➡️H2O(l); If the temperature of the system is decreased:

Powdered marble reacts more rapidly with HCl than the chips of marble because:

In the reaction: 2B ➡️Product; the rate equation is: Rate = k[B]. If the concentration of is doubled, the rate of reaction will increase by a multiple of

The reactions with the high value of energy of activation are

Of the following product-favoured processes, which are endothermic? 1. the combustion of methane to produce water and carbon dioxide. 2. the expansion of an ideal gas. 3. the melting of ice at temperatures greater than 0ºC.

If the reaction A + B C has an equilibrium constant greater than one, which of the following statements is correct?

A reaction with a negative value of 🔼G is said to be

Which of the following expressions is associated with the law of conservation of energy?

The specific heat of silver is 0.0565 $cal/g/^{o}C$. Assuming no loss of heat to the surroundings or to the container, calculate the final temperature when 100 g of silver at 40 $^{o}C$ is immersed in 60 g of water at 10 $^{o}C$.

The reactions catalyzed by sunlight are called ____________ reactions

Which of the following involves a decrease in entropy?

Every type of chemical bond contains a certain amount of energy. The total bond energy, which is essentially equivalent to the total potential energy of the system, is a quantity known as:

If a chemical reaction has a positive change in entropy, 🔼S, then

In a reaction: 2A ➡️B + 2C, which of the statement is true?

A statement of the second law of thermodynamics is that

Which of the following statements about enthalpy is incorrect?

The heat of combustion for 1 mole of carbon to carbon dioxide is -410 kJ. How many kJ of heat would be liberated from the complete combustion of 60.0 g of carbon?

All of the following statements concerning entropy are true EXCEPT

Which of the following statements about the kinetics of the reaction H2(g) + Br2(g) ➡️2HBr(g) is definitely true?

When extra NH3 is added to the following system at equilibrium: 3H2(g) + N2(g) ➡️ 2 NH3(g), what happens?

Calculate the standard entropy change for the following reaction, 2Ag2O(s) ➡️4 Ag(s) + O2(g); given S^{o}[Ag2O] = 121.3 J/K·mol, S^{o}[Ag(s)] = 42.6 J/K·mol, and S^{o}[O2(g)] = 205.1 J/K·mol.

Which reaction is likely to have a negative change in entropy?

The minimum additional energy, above the average internal energy, which the reacting molecules must possess so that their collision result in a reaction is known as

The temperature remains constant as energy is added to a substance. How may the substance be changing?

In a reaction in which the rate of the reverse reaction is equal to the rate of the forward reaction, a state of ____________ is attained.

Rusting of iron Is an example of________ reaction

Calculate the standard entropy change for the following reaction, 2 Ag2O(s) ➡️4 Ag(s) + O2(g)

given S^{o}[Ag2O] = 121.3 J/K·mol, S^{o}[Ag(s)] = 42.6 J/K·mol, and S^{o}[O2(g)] = 205.1 J/K·mol.

For a reaction: 2H2+ 2NO ➡️2H2O + N2 the rate law is R = K [H2][NO]^2 The Order of the reaction is?

Predict the signs of 🔼H and 🔼S for the evaporation of water at 35 ^oC.

If a gas absorbs 1000 J of heat and expands by 0.5 $dm^{3}$ against a constant pressure of 4 atms (1 atm = 100000 Pa), then the change in internal energy is approximately

The common-ion effect

If a process is exothermic and not spontaneous, then what must be true?

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