MDCAT Chemistry Chapter 7 MCQ Test With Answer (Chemical Equilibrium)

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MCQ's Test For MDCAT Chemistry Chapter 7 Chemical Equilibrium Online Test

Try The MCQ's Test For MDCAT Chemistry Chapter 7 Chemical Equilibrium Online Test

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MDCAT Chemistry Chapter 7 Chemical Equilibrium Online Test

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Question # 1

Which of the following processes has always. ∆H=-ve

Question # 2

One Joule is equivalent to

Question # 3

Most of the reactions which give stable products are

Question # 4

The enthalpy of formation of a compound is

Question # 5

The value of ∆V being very small. The term P∆V can be neglected for process involving

Question # 6

Enthalpy of formation of one mole of ionic compound form gaseous ion under standard condition is called

Question # 7

One of the best applications of Hess's law to calculate the lattice energy of ionic compound is

Question # 8

The enthalpy change for the reaction C2H2 + 5/2 O2 --------> 2CO2 + H2O is known as enthalpy of

Question # 9

Enthalpy of a reaction can be measured by

Question # 10

The change in enthalpy when one mole of a substance is dissolved in a specified quantity of solvent at a given temperature is called

Question # 11

What is not correct about ∆HF

Question # 12

During an exothermic or endothermic reaction which one of the following formula is used to calculate the amount of heat evolved or absorbed

Question # 13

For an endothermic reaction, enthalpy of reactants

Question # 14

Change in enthalpy (∆H) of a system can be calculated by

Question # 15

The change in enthalpy of a system when one mole of the substance is completely burnt in excess of air or oxygen is called

Question # 16

∆H=∆E is true for which of the following reaction

Question # 17

If a reaction involves only solids and liquids, which of the following is true?

Question # 18

ΔH° represent the enthalpy change at

Question # 19

Born-Haber cycle is an application of

Question # 20

The heat of reaction depends upon

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Prepare Complete Set Wise MDCAT Chemistry Chapter 7 Chemical Equilibrium Online Test MCQs Online With Answers


In this topic,Student should be able to :

a) Describe and explain redox processes in terms of electron transfer and/or of changes in oxidation number.

b) Define the terms: Standard electrode (redox) potential and Standard cell potential.

c) Describe the standard hydrogen electrode as reference electrode.

d) Describe methods used to measure the standard electrode potentials of metals or non-metals in contact with their ions in aqueous solution

e) Calculate a standard cell potential by combining two standard electrode potentials.

f) Use standard cell potentials to: i) Explain/deduce the direction of electron flow in the external circuit. ii) Predict the feasibility of a reaction.

g) Construct redox equations using the relevant half-equations.

h) State the possible advantages of developing the H2/O2 fuel cell

i) Predict and to identify the substance liberated during electrolysis from the state of electrolyte (molten or aqueous), position in the redox series (electrode potential) and concentration e.g. H2SO4(aq) and Na2SO4(aq).

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Sr.# Question Answer
1 The measurement of enthalpy change at standard conditions means that we should manage the measurement at
A. 24°C at 1 atm
B. 25°C at 1 atm
C. 0C° at 1 atm
D. 100C° 1 atm
2 Choose from the followings the correct statement about Born Haber cycle
A. Born Haber cycle is different from Hess's law
B. The energy changes in a cyclic process is not zero
C. The lattice energy of crystalline substances can be calculated easily
D. None
3 One kilo calorie is equal to
A. 4.184J
B. 1000J
C. 4184J
D. 1kJ
4 The net heat change in a chemical reaction is the same whether it is brought about in two or more different ways in one or several steps.it is known as
A. Henry's law
B. Hess's law
C. joule's law
D. Law of conservation of energy
5 The enthalpy of formation of a compound is
A. Positive
B. Either positive or negative
C. Negative
D. None
6 The exothermic process is
A. Evaporation
B. Sublimation
C. Respiration
D. Boiling
7
By convention, the standard heat of formation of all elements is assumed to be
A. Zero
B. positive
C. Negative
D. Infinity
8 The lattice energy of NaCl is
A. 787 j/ mole
B. 790 kj/mol
C. 780 kJ/ mol
D. -787 kI / mole
9 NaOH+HCI- NaCI+ H2O. Enthalpy change in the above reaction is called
A. Enthalpy of reaction
B. Enthalpy of Neutralisation
C. Enthalpy of formation
D. Enthalpy of combustion
10 The change in enthalpy of a system when one mole of the substance is completely burnt in excess of air or oxygen is called
A. Heat of reaction
B. Heat of formation
C. Heat of atomization
D. Heat of combustion

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