1st Year Chemistry Chapter 5 Thermochemistry MCQs

Here you will find the important 1st Year Chemistry Chapter 5 Thermochemistry MCQs. The branch of chemistry in which we study the heat changes during a chemical reaction. Then there is a type of energy and exothermic and endothermic reactions. The concept of Bond energy says that the average amount of energy that is required to break all bonds in one mole of a substance. The concepts of lattice energy and its measurements are also given in this chapter. Finally, two important laws including Hess’s law of constant heat summation and the Born Haber Cycle are in this chapter. So, check out the important MCQs below that you can use to practice for your entrance test. Solve the quiz below and prepare for the entry test.

1st Year Chemistry Chapter 5 Thermochemistry MCQs

445

Chemistry Chapter 5

1 / 20

Which of the following is not a state function?

Internal energy

Work

Gibb’s free energy

Enthalpy

2 / 20

A chemical change occurs when:

A shirt is ironed

Milk sours

Perfume evaporates

Electricity pass through copper wire

3 / 20

△Hn for the reaction NaOH + CH3COOH is:

57 KJ

Zero

Less than 57 KJ

More than 57 KJ

4 / 20

The smallest unit of heat energy is:

Calorie

Erg

Joule

Kilo Joule

5 / 20

In thermochemistry force-displacement work is replaced by:

Pressure volume work

Temperature volume work

Pressure temperature work

None of these

6 / 20

The conditions for standard enthalpy change are:

1 atm and 273 K

1 atm and 0 K

1 atm and 298 K

1 atm and –273° C

7 / 20

The first law of thermodynamics is represented as:

△E =q + RT

△E = q + W

△E = △H

△E = q + △P

8 / 20

The enthalpy of an element in standard states is:

1 KJ–mol–1

298 KJ–mol–1

Zero

None of these

9 / 20

In the formation of 1 mole of a compound from its element, the standard enthalpy change is called

Internal energy change

Enthalpy of formation

Enthalpy of neutralization

None of these

10 / 20

The value of DH and DE are approximately the same for the process in the case of liquids and solids because

There is no change in temperature

Volume change is negligible

Head absorbed

Heat is released

11 / 20

Neutralization of strong acid with a strong base is:

non-spontaneous reaction

Spontaneous and endothermic

Spontaneous and exothermic reaction

Non-spontaneous endothermic reaction

12 / 20

Born Haber cycle is the application of

Law of mass action

Hess’s law

Rate law

Equilibrium law

13 / 20

Which is contrary to the 1st law of thermodynamics?

Energy can never be produced

Energy can neither be formed nor destroyed

In an adiabatic process, work done is independent of its path

Continuous production of work without supply of an equivalent amount of energy

14 / 20

A calorie is equal to

0.4184 J

41.84 J

4.184 J

418.4 J

15 / 20

The formula to determine lattice energy is

△Hlatt = △Hform – △Hx

△He = △Hx –△Hf

△He = △Hf +△Hx

None of above

16 / 20

Hess’s law is used to calculate

Heat of combustion

Lattice energy

Heat of formation

All of above

17 / 20

A bomb calorimeter is used to determine

Heat of neutralization

Heat of combustion

Heat of solution

Heat of formation

18 / 20

Which of the enthalpy change is always positive

Heat of solution

Heat of neutralization

Heat of combustion

Heat of atomization

19 / 20

If the internal energy of a system increases then which of the following change may take place?

State of the system may change

Chemical reaction may take place

Temperature of the system may rise

All of the above

20 / 20

If an endothermic reaction takes rapidly in a container, the temperature of the surrounding

Increases

Decreases

Remains constant

Difficult to predict

Your score is

1st Year Chemistry Chapter 5 Thermochemistry MCQs

Related Articles

2nd Year Chemistry Chapter 14 MCQs

2nd Year Chemistry Chapter 13 MCQs

2nd Year Chemistry Chapter 11 MCQs

Post Comment Cancel reply