MDCAT CHEMISTRY-Thermochemistry (SMART INSTITUTE)
MDCAT Chemistry Thermochemistry Quiz
Test your understanding of thermochemistry concepts with our engaging MDCAT Chemistry Quiz! This quiz covers key topics including enthalpy of reactions, heat transfer, and the laws governing thermodynamic processes.
Whether you are preparing for your exams or simply want to enhance your knowledge, this quiz is designed to challenge you and solidify your grasp of important chemical principles. Here are some highlights:
- Multiple choice questions
- Detailed explanations for each answer
- Fun and educational experience
01-Enthalpy of neutralization of strong acids and strong bases have same values because
Neutralization leads to the formation of salt and water
Strong acids and bases are ionic substances
Acids always give rise to H+ bases always furnish OH- ions
The net change involves the combination of H+ and OH- ions to form water
02-For an endothermic reaction, enthalpy of reactants
Is smaller than that of the products
Is greater than that of the products
Is equal to that of the products
Must be greater or smaller than that of the products
03-WOF has positive value of enthalpy
Neutralization
Atomization
Combustiion
All of these
04-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 other several steps. It is known as:
Henry's law
Hess's law
Joule's principle
Law of conservation of energy
05-Hess's law is analogous to
Law of heat summation
Law of increasing entropy
Law of heat exchange
1st law of thermodynamics
06-NaOH + HCl → NaCl + H2O.Enthapy change in the above reaction is called
Enthalpy of reaction
Enthalpy of neutralization
Enthalpy of formation
Enthalpy of combustion
07-If a reaction involves only solids and liquids, WOF is true?
ΔH=ΔE
ΔH>ΔE
ΔH<ΔE
ΔH=ΔE+nRT
08-Calorie is equivalent to
0.4184 J
40.18 J
4.184 J
418.4 J
09-The values of H for the process I (g) + e-1 → I-1 (g) is:
>0
0
<0
None of these
10-The enthalpy of formation of a compound is
Positive
Either positive or negative
Negative
None of above
11-What is correct about heat of combustion
It is positive in some cases while negative in other
It is applicable to gaseous substances only
It is always negative
It is always positive
12-What is not correct about Hf
Its values give an idea about the relative stability of reactants and the products
It is always negative
Value depends upon nature of bonds
Its value can be greater or less than zero
13-If an endothermic reaction is allowed to take place very rapidly in air, the temperature of the surrounding air will
Remains constant
Decrease
Increase
Either increase or decrease
14-One joule is equivalent to:
4.184 cal
1/2 cal
0.4184 cal
1/4.184 cal
15-The heat of reaction depends upon
Temperature of the reactants
Physical state of the reactants and products
Both of above
Path of the reaction and the temperature
16-The exothermic process is
Evaporation
Respiration
Sublimation
Boiling
17-During an exothermic or endothermic reaction WOF formula is used to calculate the amount of heat evolved or absorbed
ΔH=ΔE+PV
Δp=ΔH
ΔE=q + w
Q=m x s x ΔT
18-Most of the reactions which give stable products are
Endothermic
Exothermic
Isothermal
None of these
19-The measurement of enthalpy change at standard conditions means that we should manage the measurement at
24 'C at 1 atm
0 'C at 1 atm
25 'C at 1 atm
100 'C at 1 atm
20-Total heat content of a system is called
Internal energy
Enthalpy
Entropy
All of these
21-The enthalpies of all elements in their standard states are
Unity
Always +ve
Always -ve
Zero
22-A state function which describes together the internal energy and products of pressure and volume is called
Enthalpy
Internal energy
Work
Kinetic energy
23-The enthalpy change for the reaction C2H2 + 5/2 O2 → 2CO2 + H2O is known as enthalpy of:
Formation of CO2
Combustion of C2H2
Fusion of C2H2
Vaporization of C2H2
24-The value of ΔV being very small. The term PΔV can be neglected for process involving
Liquid and gas
Liquid and solid
Solids and gases
None of these
25-The lattice energy of NaCl is
787 J/mol
780 J/mol
790 J/mol
-787 J/mol
26-Decomposition of H2O is
Endothermic reaction
Exothermic reaction
Nuclear reaction
Zero nuclear reaction
27-According to Hess's law, the enthalpy change for a reaction
Depends upon path
The sum of ΔE and ΔH
Independent of path
None of these
28-Enthalpy of formation of one mole of ionic compound form gaseous ion under standard condition is called
Gibb's energy
Lattice energy
Bond energy
All of these
29-Choose from the following the correct statement about Born-Haber cycle
Born Haber cycle is different from Hess's law
The energy changes in a cyclic process is not zero
The lattice energy of crystalline substances can be calculated easily
None of these
30-Change in enthalpy (ΔH) of a system can be calculated by
ΔH=ΔE -PV
ΔH=ΔE -q
ΔH=ΔE + q
ΔH=ΔE + PΔV
31-If internal energy of the system is increased
Change in the state of system may occur
Temperature of the system may rise
Chemical reaction may take place
All of these
32-Enthalpy of a reaction can be measured by
Glass calorimeter
Baroometer
Manometer
Thermometer
33-In order to determine ΔHlatt. of ionic compound which is correct relationship
ΔH latt. = ΔHf - ΔHx
ΔH latt. = ΔHf + ΔHx
ΔH latt. = ΔHa + ΔHv
ΔH latt. = ΔHf - ΔHsol
34-Enthalpy of neutralization (ΔHn) per mole of H2SO4 / Ba(OH)2 is
-57.4 kJmol-1
-114.8 kJmol-1
+57.4 kJmol-1
+114.8 kJmol-1
35-Whenever a reaction is endothermic, then it means that
Heat heat is transferred from surrounding to the system
Heat is transferred system to surrounding
Heat content if the products is less than that of reactants
Heat content of the reactants is greater than the products
36-How much heat is absorbed by 100 g of water when its temperature decreases from 25'C to 5'C? ( heat capacity is 4.2 J/gK)
84000 J
2000/4.2 J
-2000/4.2 J
-8400 J
37-One of the best applications of Hess's law to calculate the lattice energy of ionic compound is
Measurement of enthalpy change in a calorimeter
Studying of the law of Thermodynamics
Born-Haber cycle
Measurement of a heat of formation of a compound
38. ΔH of a system can be calculated by WOF relationship
Q = m x s x ΔT
Q = m x v x ΔT
Q = ΔE
Q = pv
39-WOF processes have always ΔH = -ve
Formation of compound
Dissolution of ionic compound
Combustion
Dilution of a solution
40. ΔH = ΔE is true for WOF reaction
K(s) + H2O(l) → KOH(aq) + H2(g)
N(g) + 3H2(g) ⇌ 2NH3(g)
AlCl3(aq) +3NaOH(aq) → Al(OH)3(aq) +3NaCl(aq)
4Na(s) + O2(g) → 2Na2O(s)
41. BaCl2(aq) + H2SO4(aq) → BaSO4(s) + HCl(aq) ΔH = -22.4 kJ/mol, the heat change represented by above equation is called
Heat of formation of BaSO4
Heat of reaction of BaSO4
Heat of dissociation of BaSO4
Sum of all the above heats
42-When water is added to quicklime, the reaction is
Explosive
Endothermic
Exothermic
Photochemical
43. In an endothermic reaction
E(R) > E(P)
E(R) = E(P)
E(R) < E(P)
NONE OF THESE
44. What type of reaction constitute a limiting case between spontaneous and non-spontaneous reaction
Irreversible reaction
Nuclear reaction
Reversible reaction
Thermal reaction
45.Thermodynamics does not deal with
Heat of reaction
Rate of reaction
Spontaneity of reaction
Entropy of reaction
46 ............... Is not a state function.
Enthalpy
Temperature
Internal energy
Heat
47. The enthalpy of atomization of H2(g) is 218 kJ/mol, the enthalpy of formation of H2(g) from gaseous atoms
1/2H2(g) → ΔHat = 218 kJmol-1
-218 kJ/mol
+436 kJ/mol
-436 kJ/mol
+218 kJ/mol
48-The enthalpy change for the reaction C(s) + O2(g) → CO2(g) is called
Enthalpy of formation
Enthalpy of reaction
Enthalpy of combustion
All of these
49-A process which is spontaneous and endothermic
H2O(l) → H2O(g)
N2(g) + O2(g) → 2NO(g)
H2O(g) → H2O(l)
NaOH + HCl → NaCl + H2O
50-Which equation shows lattice energy for ionic compound
Na(s) + 1/2 Cl2(g) → NaCl(s)
Na(s) + Cl(g) → NaCl(s)
Na(aq) + Cl-(aq) → NaCl(aq)
Na(g) + Cl-(g) → NaCl(s)
51-An enthalpy change which is always exothermic
ΔH at
ΔH solution
ΔH n
ΔH f
52-All of the following are exothermic process except
Freezing of water
Evaporation
Condensation
Combustion
53-Enthalpy of combustion of food, fuel and other compound can be measured accurately by
Glass calorimeter
Thermometer
Bomb calorimeter
Manometer
54-The enthalpy of formation of an ionic compound is -392 kJ/mol. Total energy changes (ΔHx) involved in the formation of gaseous ions from normal physical state is 280 kJ/mol. The enthalpy of lattice (ΔH latt.) is
-112 kJ/mol
-672 kJ/mol
+672 kJ/mol
=224 kJ/mol
55-WOF enthalpies of formation cannot be measured directly
ΔH latt. For ionic compound
ΔHf for B2O3
ΔHf for CO
ALL OF THESE
56-All are slow processes except
Fermentation of sugar
Weathering of rocks
Reaction of AgNO3 with NaCl
Rusting of iron
57-Heat absorbed or evolved during the chemical reaction at constant pressure is
ΔH
ΔV
ΔE
ΔH+ΔE
58-Bomb calorimeter is used to determine the
ΔH s
ΔH I
ΔH c
ΔH n
59-Which enthalpy of reaction cannot be determined by glass calorimeter
Enthalpy of formation
Enthalpy of solution
Enthalpy of neutralization
Enthalpy of combustion
60-Which is not related to state function
It is a macroscopic property
It deals with atomic level
It depends upon initial and final values
It is independent of path
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