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

Total heat content of a system is called

Question # 2

By convention, the standard heat of formation of all elements is assumed to be

Question # 3

The lattice energy of NaCl is

Question # 4

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

Question # 5

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

Question # 6

Decomposition of H2O is

Question # 7

What is not correct about ∆HF

Question # 8

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

Question # 9

Enthalpy of neutralization of strong acids and strong bases have same values because

Question # 10

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

Question # 11

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

Question # 12

Born-Haber cycle is an application of

Question # 13

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

Question # 14

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

Question # 15

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

Question # 16

Most of the reactions which give stable products are

Question # 17

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

Question # 18

For an endothermic reaction, enthalpy of reactants

Question # 19

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

Question # 20

Whenever a reaction is endothermic, then it means that

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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 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
2 If a reaction involves only solids and liquids, which of the following is true?
A. ΔH = ΔE
B. ΔΗ =ΔΕ
C. ΔH>ΔΕ
D. AH =AE +nRT
3 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
4 Which of the following has positive value of enthalpy
A. Neutralisation
B. Atomization
C. combustion
D. All of the above
5 The value of ∆V being very small. The term P∆V can be neglected for process involving
A. Liquid and gas
B. Solids and gases
C. Liquid and solid
D. None of these
6 A system absorbs 100 kJ heat and performs 50 kJ work on the surroundings. The increase in internal energy of the system is
A. 50kJ
B. 100 kJ
C. 150kJ
D. 5000 kJ
7 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
8
By convention, the standard heat of formation of all elements is assumed to be
A. Zero
B. positive
C. Negative
D. Infinity
9 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
10 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
11 The enthalpy change AH of a process is given by the relation
A. ΔΗ =ΔΕ + P∆V
B. ΔH=ΔE +W
C. ΔH =ΔΕ-ΔnRT
D. ΔΕ =ΔΗ + P∆V
12 According to Hess's law, the enthalpy change for a reaction
A. Depends on path
B. Independent of the path
C. The sum of ∆E and ∆H
D. None of these
13 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
14 The enthalpy of formation of a compound is
A. Positive
B. Either positive or negative
C. Negative
D. None
15 A state function which describes together the internal energy and product of pressure and volume is called
A. Enthalpy
B. internal energy
C. Work
D. Kinetic energy
16 What is not correct about ∆HF
A. It is always negative
B. Ìts value gives an idea about the relative stability of reactants and the products.
C. Its value can be greater or less than zero
D. Value depends upon nature of bonds
17 The lattice energy of NaCl is
A. 787 j/ mole
B. 790 kj/mol
C. 780 kJ/ mol
D. -787 kI / mole
18 If an endothermic reaction is allowed to take place very rapidly in air, the temperature of the surrounding air will
A. Remains constant
B. Increase
C. Decrease
D. Either increase or decrease
19 The values of ∆H for the process l(g)+e-1--------->
I-1(g) is:
A. >0
B. <0
C. 0
D. None
20 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

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