Chemistry Chapter 6 Mock Test

From a temperature of 27°c, one mole of an ideal gas is allowed to expand reversibly and adiabatically. If the work done during the process is 3 kJ, the final temperature will be equal to (C_v = 20JK-¹)

295 K
150 K
100 K
26.85°C

The enthalpy of neutralization _______ of acid and bases is nearly same.

HCI and NaCI
HCI and KOH
HCN and NaOH
HCI and NH40H

The bond that possess the highest average bond energy (Kcal/mol) is:

N \(\equiv \)N
C \(\equiv \) N
C \(\equiv \) C
S = O

System absorbs 600 J of heat and work equivalent to 300 J on its surroundings. Find the change in internal energy.

600 J
500 J
400 J
300 J

The volume must be expressed in which of the following term in order to calculate the amount of work done in joules during reversible isothermal expansion of an ideal gas

\(cm^3 \) only
\(m^3 \) only
\(dm^3\) only
any one of them

Mutual heat of neutralization of 40 gm of Sodium hydroxide (NaOH) and 60 gm Acetic acid (CH₃COOH) will be

less than 56.1 kcal
56.1 kcal
more than 56.1 kcal
13.7 kcal

Values of \(\Delta \)H for the combustion of ethene and ethyne are – 341.1 and – 310.0 kcal respectively. Which one of the following is a better fuel?

\(C_2H_4\)
\(C_2H_4\)
Both of these
None of these

When disorder of a system increases, the change is known to be:

spontaneous
endothermic
exothermic
non-spontaneous

8 gm of methane (CH₄) is completely burnt in air. Find the no. of moles of water produced.

18
2
1
0.5

Statement 1 : T, P and V are state variables or state functions.

Statement 2 : Their values depends upon the state of system and how it is reached.

Both statement 1 and statement 2 are true and the statement 2 is the correct explanation of the statement 1
Both statement 1 and statement 2 are true but statement 2 is not the correct explanation of the statement 1
Statement 1 is true but statement 2 is false
The statement 1 and statement 2 both are false

Variation of heat of reaction with temperature is called as

Van't Hoff isochore
Van't Hoff isotherm
Kirchoff’s equation
Kemmerling equation

Enthalpy of formation of ammonia is 46.0 kJ\(mol^{-1}\) Find the enthalpy change for the reaction 2NH₃(g) \(\to\) 2N₂(g) + 3H₂(g).

-92.0 kJ \(mol^{-1}\)
– 23.0 kJ \(mol^{-1}\)
92.0 kJ \(mol^{-1}\)
46.0 kJ [latex]mol^{-1}[/latex]

The combustion of 5.0 of coke raised the temperature of 1 kg of water from 10°C to 47°C. Estimate the fuel value of coke in kcal/g.

7.4 kcal/g
8.4 kcal/g
6.4 kcal/g
9.4 kcal/g

The condition in which a chemical reaction can not occur is:

\(\Delta \) H decreases and \(\Delta \) S increases
\(\Delta \)H increases and \(\Delta \)S decreases
\(\Delta \)H and \(\Delta \)S decrease and \(\Delta \)H >T\(\Delta \)S
\(\Delta \)H and \(\Delta \)S increase and T\(\Delta \)S > \(\Delta \)H

Find the amount of work done during the expansion of a gas from a volume of 4dm³ to 6dm³ against a constant external pressure of 3atm? (1L atm = 101.32 J)

-6 J
-608 J
-304 J
+304 J

Statement 1: Heat of sublimation is the sum of heat of fusion and the heat of vaporization.

Statement 2: Heat of reaction or enthalpy change is same whether the reaction takes place in one step or in a no. of steps.

Both Statement 1 and Statement 2 are true but Statement 2 is not the correct explanation of Statement 1
Both Statement 1 and Statement 2 are true and the Statement 2 is correct explanation of the Statement 1
This Statement 1 is true, but the Statement 2 is false
Both Statement 1 and Statement 2 are false

The condition that will always lead to a non-spontaneous change is:

Positive \(\Delta \)H and negative \(\Delta \)S
Positive \(\Delta \)H and positive \(\Delta \)S
Negative \(\Delta \)H and negative \(\Delta \)S
Negative \(\Delta \)H and positive \(\Delta \)S

The weight of oxygen which is required for the complete combustion of 2.8 kg of ethylene is:

2.8 kg
6.4 kg
9.6 kg
96.0 kg

Entropy of crystalline substances at absolute zero going according to the third law of thermodynamics should be taken as

50
100
Zero
Different for different substances

The value of \(\Delta H\) in an endothermic reaction is

constant
negative
positive
zero

Find the amount of work done during isothermal expansion of one mole of an ideal gas from 10 atm to 1 atm at 300 K.

4138.8 J
4938.8 J
5744.1 J
6257.2 J

C (diamond) + C₂(g) \(\to \) CO₂(g); \(\Delta H\) = -395 kJ

C (graphite)-O₂ (g) \(\to \) CO₂(g); \(\Delta H\) = -393.5 kJ

From the data, the \(\Delta H\) when diamond is formed from graphite, is

-3.0 kJ
+3.0 kJ
+1.5 kJ
-1.5 kJ

Statement 1 : At constant temperature and constant volume, heat absorbed in a reaction is -\(\Delta G \).

Statement 2 : For the reaction to be spontaneous, \(\Delta G \) should be negative.

Both statement 1 and statement 2 are true and the statement 2 is the correct explanation of the statement 1
Both statement 1 and statement 2 are true but statement 2 is not the correct explanation of the statement 1
Statement 1 is true but statement 2 is false
Statement 1 is false but statement 2 is true

Which one of the following statement is correct

The enthalpy of fusion is negative
The heat of neutralization of strong acid and strong base is always the same
\(\Delta H\) is negative for endothermic reaction
\(\Delta H\) is positive for exothermic reaction

Law of thermodynamics which helps in calculating entropy at different temperatures is

Zeroth law
First law
Second law
Third law

Carbon and carbon monoxide burn in oxygen to form carbon dioxide as per the following reactions

C + O₂ \(\to \)CO₂; \(\Delta H \) = – 394 kJ mol^-1

2CO + O₂ \(\to \) 2CO₂; \(\Delta H \) = – 569 kJ mol^-1

Find the heat of formation of 1 mol of carbon monoxide.

– 87.5 kJ mol-1
– 109.5 kJ mol-1
– 175.0 kJ mol-1
– 219.0 kJ mol-1

Statement 1 : Entropy of ice is less than that of water.

Statement 2 : Ice possess cage like structure.

Both statement 1 and statement 2 are true and the statement 2 is the correct explanation of the statement 1
Both statement 1 and statement 2 are true but statement 2 is not the correct explanation of the statement 1
Statement 1 is true but statement 2 is false
The statement 1 and statement 2 both are false

Find the correct one for the phase transition of 1 mol of H₂O . H₂O_{s)⇌ H₂O_{1) at 0°C and 1 atm

\(G_{ice} = G_{water} \) = 0
\(G_{ice} = G_{water} \) \(\ne \) 0
\(G_{ice} > G_{water} \)
\( G_{ice} > G_{water} \)

Gibbs free energy G, enthalpy H and entropy S are interrelated as in which of the following?

G = S = H
G -TS = H
G = H – TS
G = H + TS

Find molar heat capacity of water in equilibrium with ice at the constant pressure.

75.48 J \(K^{-1} \)
40.45 kJ\(K^{-1} \) \(mol^{-1} \)
Infinity( \( \propto \))
0

The densities of graphite and diamond at 298 K are 2.25 and 3.31 g cm-³, respectively. Find the pressure at which graphite will be transformed diamond at 298 K if the standard free energy difference (\(\Delta \)G°) is equal to 1895 J mol^-1

9.92 x l08 Pa
9.92 x l07 Pa
9.92 x l06 Pa
9.92 x l05 Pa

Which one of the following would be expected to possess the largest entropy per mole?

\(SO_{2}(g)\)
\(SO_2Cl_2(l)\)
\(SO_2Cl_2(g)\)
\(SO_2Cl_2(s)\)

Bond dissociation energy required to form benzyl radical from toluene is _______ than the formation of the methyl radical from methane

much
less
equal
none of the above

Which one of the following is least random state of water?

Liquid water
Ice
Steam
All present same random state

For the determination of heat of ________ Hess law is applicable

formation
reaction
transition
all of these

The equation which gives the dependence of Gibbs free energy on pressure for an isothermal process of an ideal gas is:

\(\Delta G_T = nRT log \frac{V_2}{V_1}\)
\(\Delta G_T = nRT log \frac{P_2}{P_1}\)
\(\Delta G_T = nRT In\frac{V_2}{V_1}\)
\(\Delta G_T = nRT In \frac{P_2}{P_1}\)

In which of the following, maximum entropy is present?

Water vapours
Snow
Liquid water
Ice

Which of the following is correct for the exothermic reaction?

\(\Delta H\) is always positive
H of the products is equal to H of the reactants
H of the products is more than H of the reactants
H of the products is less than H of the reactants

In which of the following state, the matter possess highest entropy?

Gas
Solid
Liquid
Equal in all

2.1 g of Iron (Fe) combines with Sulphur (S) evolving 3.77 kJ. Find the heat of formation of FeS in KJ/mol.

-100.5
-1.79
-3.77
None of these

Which of the following is (are) endothermic reaction?

Dehydrogenation of ethane to ethylene
Decomposition of water
Conversion of graphite to diamond
All of above

The enthalpy of solution of BaCl₂(s) and BaCl₂.2H₂O(s) are -20.6 and 8.8 kJ mol^-1 Find the enthalpy change for the reaction BaCl₂(s) + 2H₂O \(\to \)

-29.4 kJ
-20.6 kJ
-11.8 kJ
29.4 kJ

_______ condition is not favourable for the feasibility’ of a reaction.

\(\Delta H\)= -ve \( T \Delta S\)= +ve
\(\Delta H\)= +ve \( T \Delta S\)= + ve and \( T \Delta S\) > \(\Delta H\)
\(\Delta H\)= +ve \( T \Delta S\)= + ve and \( T \Delta S\) < \(\Delta H\)
\(\Delta H\)= +ve \( T \Delta S\)= – ve and \( T \Delta S\) < \(\Delta H\)

The entropy changed involved in the conversion of 1 mole of liquid water at 373 K to vapour at the same temperature will be [\(\Delta \)H_vap = 2.257kJ / gm]

0.129 kJ/mol/K
0.120 kJ/mol/K
0.119 kJ/mol/K
0.109 kJ/mol/K

For the determination of heat of ______ Hess law is applicable.

formation
reaction
transition
all of these

Chemistry Class 11 QBank

Tests

Chemistry Chapter 6 Mock Test

Test Summary

Information

Results

Results

Categories

1. Question

2. Question

3. Question

4. Question

5. Question

6. Question

7. Question

8. Question

9. Question

10. Question

11. Question

12. Question

13. Question

14. Question

15. Question

16. Question

17. Question

18. Question

19. Question

20. Question

21. Question

22. Question

23. Question

24. Question

25. Question

26. Question

27. Question

28. Question

29. Question

30. Question

31. Question

32. Question

33. Question

34. Question

35. Question

36. Question

37. Question

38. Question

39. Question

40. Question

41. Question

42. Question

43. Question

44. Question

45. Question