Thermodynamics ...

Direction (Q. Nos. 1- 8) This section contains 8 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE option is correct.

Q. For the given reaction, = - 1.3818 kcal at 300 K. Thus equilibrium constant is

ΔH_vap = 30 kJ mol^-1 and ΔS_vap = 75 J mol^-1 K^-1. Thus, temperature of vapour at one atmosphere is

[IIT JEE 2004]

Which reaction, with the following values of ΔH and ΔS at 400 K is spontaneous and endothermic?

Standard entropies of X₂, Y₂ and XY₃ are given below the reaction

Q. At what temperature, reaction would be in equilibrium? 

The value of log₁₀ K for a reaction, A B is (Given, ΔH°₂₉₈ = - 54.07 kJ mol^-1;

ΔS°₂₉₈ = + 10 JK^-1 mol^-1; R = 8.314 JK^-1 mol^-1 2.303 x 8.314 x 298 = 5705) 

[IITJEE2007]

For the following decom position reaction, 

ΔG° = 1729 J mol^-1 at 300 K , (log 5 = 0.6990]

Thus, pressure set up is

If for the cell, Zn(s) + Cu²⁺(ag) Cu(s) + Zn²⁺ (ag)entropy change ΔS° is 96.5 JK^-1 mol^-1, then temperature coefficient of the emf of a cell is

For the reaction, at 1000° C

ΔG° = - 27 kJ mol^-1,  = 0.0033 atm.

Q. Hence, ΔG at this temperature is

Direction (Q. No. 9) This sectionis based on statement I and Statement II. Select the correct answer from the code given below.

Q. 

Statement I :Every endothermic reaction is spontaneous if TΔS > ΔH.

Statement II : Sign of ΔG is the true criterion for deciding spontaneity of a reaction.

Direction (Q. Nos. 10) Choice the correct combination of elements and column I and coloumn II  are given as option (a), (b), (c) and (d), out of which ONE option is correct.

Q. Thermodynamic equilibrium constant K is related to temperature by equation log₁₀