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

00:00
Question # 1

NaOH+HCI- NaCI+ H2O. Enthalpy change in the above reaction is called

Question # 2

The enthalpy change AH of a process is given by the relation

Question # 3

Calorie is equivalent to

Question # 4

Neutralization of acid-base is

Question # 5

The heat of reaction depends upon

Question # 6

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 # 7

Enthalpy of neutralization (∆H°n) per mole of H2SO4/ Ba(OH)2 is

Question # 8

What is correct about heat of combustion

Question # 9

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

Question # 10

If an endothermic reaction is allowed to take place very rapidly in air, the temperature of the surrounding air will

Question # 11

Born-Haber cycle is an application of

Question # 12

Which of the following has positive value of enthalpy

Question # 13

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

Question # 14

One Joule is equivalent to

Question # 15

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

Question # 16

The exothermic process is

Question # 17

A system absorbs 100 kJ heat and performs 50 kJ work on the surroundings. The increase in internal energy of the system is

Question # 18

One kilo calorie is equal to

Question # 19

According to Hess's law, the enthalpy change for a reaction

Question # 20

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

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


Topic Test

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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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MCAT Chemistry Chapter 7 Important MCQ's

Sr.# Question Answer
1 For an endothermic reaction, enthalpy of reactants
A. Is smaller than that of the products
B. Is greater than that of the products
C. Must be greater or smaller than that of the products
D. Is equal to that of the products
2 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
3
By convention, the standard heat of formation of all elements is assumed to be
A. Zero
B. positive
C. Negative
D. Infinity
4 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
5 Enthalpy of formation of one mole of ionic compound form gaseous ion under standard condition is called
A. Gibb's energy
B. Gibb's energy
C. Bond energy
D. Lattice energy
6 Enthalpy of a system can be calculated by which of following relationship
A. q=ΔΕ
B. q=m×S×∆T
C. q=pv
D. q=m×v×∆T
7 If internal energy of the system is increased
A. Change in state of the system may occur
B. Temperature of the system may rise
C. Chemical reaction may take place
D. All of these
8 One kilo calorie is equal to
A. 4.184J
B. 1000J
C. 4184J
D. 1kJ
9 The heat of reaction depends upon
A. Temperature of the reactants
B. Physical states of the reactants and the products
C. Both A) and B)
D. Path of the reaction and the temperature
10 Which of the following processes has always. ∆H=-ve
A. Formation of compound
B. Dilution of a solution
C. Dissolution of ionic compound
D. Combustion

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  • faisal

    faisal

    19 Jun 2019

    mdcat

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