AIIMS Chemistry Thermodynamics Class 11 Questions

C + O₂(g) ⟶ CO₂ ...... (i); ΔH = -393 kJ mol⁻¹ H₂ + 1/2 Ω₂ ⟶ H₂O ...... (ii); ΔH = -287.3 kJ mol⁻¹ 2CO₂ + 3H₂O ⟶ C₂H₅OH + 3O₂ ...... (iii); ΔH = 1366.8 kJ mol⁻¹ Find the standard enthalpy of formation of C₂H₅OH(l)

In isolated system, find the condition for spontaneous reaction:

At 25°C 1 mole of butane is heated then CO₂ and H₂O liquid is formed work done is :

One monatomic gas is expanded adiabatically from 2 L to 10 L at 1 atm external pressure, find ΔU (in atm L)?

Which of the following are extensive properties?

The factor of ΔG values is important in metallurgy. The ΔG values for the following reactions at 800°C are given as S₂(g) + 2O₂(g) → 2SO₂(g); ΔG = -544kJ 2Zn(s) + S₂(g) → 2ZnS(s); ΔG = -293kJ 2Zn(s) + O₂(g) → 2ZnO(s); ΔG = -480kJ The ΔG for the reaction, 2ZnS(g) + 3O₂(g) → 2ZnO(g) + 2SO₂(g) will be

Order nucleophilicity: (i) OH^- (ii) HS^- (iii) Ph-O^- (iv) C2H5-O^-

ΔG versus T plot in the Ellingham’s diagram slopes downward for the reaction

C₃H₆ + H₂ → C₃H₈ ΔH₁ = -224 C₃H₈ + 5O₂ → 3CO₂ + 4H₂O ΔH₂ = -2027 H₂ + ½ O₂ → H₂O ΔH₃ = -282 Calculate the combustion of propene

Which of the following is a pair of diamagnetic complex?

Assertion: The surface tension of water is more than other liquid. Reason: Water molecules have strong inter molecular H- bonding as attractive force.

Assertion: Addition of Q and w give ΔU Reason: Addition of two path function can not give state function.

Assertion: Second ionization enthalpy will be higher than the first ionization enthalpy.

In the following questions a statement of Assertion (A) followed by a statement of Reason (R) is given. Choose the correct answer out of the following choice. Assertion (A) Black body is an ideal body that emits and absorb radiations of all frequencies. Reason (R) The frequency of radiations emitted by a body goes from lower frequency to higher frequency with an increase in temperature.

Assertion: A reaction which is spontaneous and accompanied by decrease of randomness must be exothermic. Reason: All exothermic reactions are accompanied by decrease of randomness.

Arrange the given set of compounds in order of increasing boiling points. I.¹⁻chloropropane II. Iso-propyl chloride III.¹⁻chlorobutane

The factor of ΔG values is important in metallurgy. The ΔG values for the following reactions at 800°C are given as S₂(g) + 2O₂(g) → 2SO₂(g); ΔG = −544 kJ 2ZnS(s) + 3O₂(g) → 2ZnO(s) + 2SO₂(g) will be

Assume each reaction is carried out in an open container. For which reaction ΔH = ΔE?

Assertion: A process for which ΔS_syst. > 0 as well as ΔH > 0, passes from non-spontaneous to spontaneous state as temperature is increased. Reason: At higher temperature, TΔS exceeds ΔH.

Which thermodynamic parameter is not a state function?

Assertion: For an isolated system, q is zero. Reason: In an isolated system, change in U and V is zero.

Assertion: Entropy of system increases for a spontaneous reaction. Reason: Enthalpy of reaction always decreases for spontaneous reaction.

Assertion: A process is called adiabatic if the system does not exchange heat with the surroundings. Reason: It does not involve increase or decrease in temperature of the system.

At equilibrium which is correct?

For adiabatic process, which is correct?

Which of the following is not a thermodynamic function?

Which of the following is intensive property?

Assertion : Entropy is always constant for a closed system. Reason : Closed system is always reversible.

Match List I with List II and select the correct answer using the codes given below the lists:

The variation of volume V, with temperature T, keeping pressure constant is called the coefficient of thermal expansion (α) of a gas i.e., α = (1/V)(∂V/∂T)P. For an ideal gas α is equal to

In an isobaric process, when temperature changes from T₁ to T₂, ΔS is equal to

In P versus V graph, the horizontal line is found in which ______ exists.

Calculate change in internal energy if ΔH = –92.2 kJ, P = 40 atm and ΔH/ΔV = –1 L.

ΔHₓₓₓₓ of a substance is 'x' and ΔHₓₓₓₓ is 'y', then ΔHₓₓₓₓₓₓ will be

ΔSₛᵤᵣ for an exothermic reaction is

For a spontaneous process the correct statement is

For a phase change H₂O (l) ⇌ H₂O (s) at 0°C, 1 bar

The enthalpy change (ΔH) for the reaction, N₂ (g) + 3H₂ (g) → 2NH₃ (g) is^{-92}.38 kJ at 298 K. The internal energy change ΔU at 298 K is

ΔHf° (298 K) of methanol is given by the chemical equation

For the reaction of one mole of zinc dust with one mole of sulphuric acid in a bomb calorimeter, ΔU and w correspond to

Which of the following is arranged in the increasing order of enthalpy of vaporization?

Which one of the following has ΔS° greater than zero?

If P is pressure and ρ is density of a gas, then P and ρ are related as

The enthalpy change for the following reaction NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(l) is –57 kJ. Predict the value of the enthalpy change in the following reaction. Ba(OH)₂ + H₂SO₄(aq) → BaSO₄(s) + 2H₂O(l)