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

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

Question # 2

The enthalpies of all elements in their standard states are

Question # 3

In order to determine ∆H (latt) of ionic compound which is correct relationship

Question # 4

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

Question # 5

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

Question # 6

Hess's law is analogous to

Question # 7

ΔH° represent the enthalpy change at

Question # 8

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

Question # 9

Enthalpy of a reaction can be measured by

Question # 10

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

Question # 11

What is correct about heat of combustion

Question # 12

Most of the reactions which give stable products are

Question # 13

One Joule is equivalent to

Question # 14

One kilo calorie is equal to

Question # 15

Enthalpy of a system can be calculated by which of following relationship

Question # 16

The values of ∆H for the process l(g)+e-1--------->
I-1(g) is:

Question # 17

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

Question # 18

Which of the following has positive value of enthalpy

Question # 19

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

Question # 20

Total heat content of a system is called

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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 Class Chemistry Chapter 7 Important MCQ's

Sr.# Question Answer
1 One Joule is equivalent to
A. 4.184 cal.
B. 0.4184cal.
C. 1/2 cal.
D. 1/4.184 cal
2 One of the best applications of Hess's law to calculate the lattice energy of ionic compound is
A. Measurement of enthalpy change in a calorimeter
B. Studying of first law of thermodynamics
C. Measurement of a heat of formation of a compound
D. Born-Haber cycle
3 What is correct about heat of combustion
A. It is applicable to gaseous substances only
B. It is always negative
C. It is always positive
D. It is positive in some cases while negative in other
4 The enthalpy change for the reaction C2H2 + 5/2 O2 --------> 2CO2 + H2O is known as enthalpy of
A. Fomation of CO2
B. Fusion ofC2H4
C. Combustion of C2H4
D. Vaporization of C2H2
5 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
6 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
7 ∆H=∆E is true for which of the following reaction
A. K+H2O----->KOH+H2
B. N2+3H2------>2NH3
C. AlCl3+3NaOH--->Al(OH)3+3 NaCl
D. 4Na + O2----->2Na2O
8 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
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
By convention, the standard heat of formation of all elements is assumed to be
A. Zero
B. positive
C. Negative
D. Infinity

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