Chemistry chapter 8 Entry Test MCQs
101. All of the following processes do not represent hydration except
a. Na+(g) +I-(g)———>NaI(s)
b. K+(g) + Cl–(g)——->KCl(s)
c. Na+(g) +Cl–(g)———>NaCl(s)
d. K+(g) + Br–(g)———>KBr(aq)
102. Heat supplied to a system at constant pressure increases its
a. Enthalpy
b. Internal energy
c. Temperature
d. Volume
103. Calorimeter is an apparatus used for the measurement of
a. Order of the reaction
b. Mechanism of the reaction
c. Stoichiometry of the reaction
d. Heat of the reaction
104. Enthalpy of combustion for food fuel and other compounds can be measured accurately by?
a. bomb calorimeter
b. glass calorimeter
c. manometer
d. thermometer
105. Enthalpy of neutralization is merely
a. heat of combustion
b. heat of solution
c. heat of formation of H2O
d. heat of atomization
106. Conditions under which standard enthalpy changes are measured are
a. -273 0C and 1 atm
b. 273 K and 1 atm
c. 25 0C and 1 atm
d. 0 0C and 1 atm
107. The specific heat capacity of water is 4.18 JK-1g-1. What is the enthalpy change when 10g of water is heated from 285 to 300K.
a. 2.79 J
b. 627 kJ
c. 627 J
d. 6.27 KJ
108. Equal volumes of methanoic acid and sodium hydroxide are mixed. If x is the heat of formation of water, then heat evolved on neutralisation is:
a. Twice of x
b. More than x
c. Less than x
d. Equal to x
109. What is the weight of oxygen that is required for the complete combustion of 2.8 kg of ethylene?
a. 6.4 kg
b. 9.6 kg
c. 2.8 kg
d. 96.0 kg
110. ΔHᵣ is the standard enthalpy change of which of the following process?
a. When 1 mole of Reactants are converted into products
b. When 1 mol of compound formed from its elements
c. When 1 mole of salt is formed
d. When 1 mole of substance is dissolved to make a solution
111. What is the enthalpy of solution of NH4Cl?
a. 16.2 Kj/mol
b. Kj/mol
c. -16.2 Kj/mol
d. -17 Kj/mol
112. ΔH of a system can be calculated by which of the following relationship
a. q=m x v x ΔT
b. q=m x s x ΔT
c. q = pv
d. q=ΔE
Hess`s Law
113. Hess law is a simple application of
a. Law of conservation of energy
b. Law of Mass Action
c. Dalton’s Law of partial pressure
d. Law of conservation of mass
114. Standard enthalpy of Al2O3 cannot be measured because:
a. it reacts with CO2
b. it does not catch fire
c. It is not prepared directly
d. protective layer of oxide cover the surface
115. The internal energy change a system goes from state A to B is 40 KJ/mol. if the system returns from B to state A, what would be the net change in internal energy?
a. > 40 KJ
b. 40 kJ
c. Zero
d. < 40 Kj
116. “The amount of heat evolved or absorbed in a chemical reaction is the same no matter the reaction takes place in one step or several steps” is statement of
a. Law of mass action
b. First law of thermodynamics
c. Raoult’s law
d. Hess’s law
117. Hess law is applicable for the determination of heat of
a. Formation
b. Reaction
c. Transition
d. All of these
118. Hess law of heat summation includes
a. Initial reactants and final products
b. Initial reactants only
c. Intermediates only
d. Final products only
119. Formation of carbon dioxide hinders in calculating the heat of formation of
a. CO
b. CCl4
c. C
d. O3
120. Choose from the following the correct statement about Born Habor cycle:
a. The lattice energy of crystalline substances can be calculated easily
b. Born Harbor cycle is different from Hess’s law
c. It is applied for M2X compounds
d. The energy changes in a cyclic process is not zero
121. Due to the formation of protective layer of oxides at Al2O3 surface, it is hard to burn it
a. completely in oxygen
b. completely in air
c. with nitrogen
d. with carbon
122. The lattice energy is maximum for
a. MgF2
b. KF
c. CaF2
d. NaF
123. Born Haber’s cycle enables us to calculate:
a. Heat of hydration
b. Heat energy
c. Heat of solution
d. Lattice energy
124. Lattice energy helps to explain all of the following properties of ionic compounds EXCEPT:
a. Properties
b. Structure
c. Dipole Moment
d. Bonding
125. Born–Haber cycle is an application of
a. second law of thermodynamics
b. first law of thermodynamics
c. Hess’s law
d. first law of thermochemistry