The standard Gibbs energy for the given cell reaction in kJ mol-1

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251.

For silver, CP( K-1 mol-1) = 23 + 0.01T. If the temperature (T) of 3 moles of silver is raised from 300 K to 1000 K at 1 atm pressure, the value of H will be close to :

  • 21 kJ

  • 62 kJ

  • 16 kJ

  • 13 kJ


252.

Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas? (Assume non-expansion work is zero)

  • Isothermal process : q = -w

  • Cyclic process : q = -w

  • Isochoric process : U = q

  • Adiabatic process : U = -w


253.

During compression of a spring the work done is 10 kJ and 2 kJ escaped to the surroundings as heat. The change in internal energy, U (in kJ) is:

  • -12

  • 8

  • 12

  • -8


254.

Consider the given plot of enthalpy of the following reaction between A and B. A + B → C + D. Identify the incorrect statement.

  • C is the thermodynamically stable product.

  • Formation of A and B from C has highest enthalpy of activation.

  • Activation enthalpy to form C is 5 kJ mol-1 less than that to form D.

  • D is kinetically stable product.


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255.

5 moles of an ideal gas at 100 K are allowed to undergo reversible compression till its temperature becomes 200 K. If CV = 28 J K–1 mol–1, calcuIate ΔU and ΔPV for this process. ( R= 8.0 JK-1 mol-1 )

  • ΔU = 14kJ; Δ(pV) = 18kJ

  • ΔU = 14kJ; Δ(pV) = 0.8J

  • ΔU = 14kJ; Δ(pV) = 4kJ

  • ΔU = 2.8kJ; Δ(pV) = o.8J


256.

Among the following, the set of parameters that represents path functions, is:

(A) q+w

(B) q

(C) w

(D) H-TS

  • A, B and C

  • B, C and D

  • B and C

  • A and D


257.

A process will be spontaneous at all temperatures if :

  • ΔH <0 and ΔS <0

  • ΔH <0 and ΔS >0

  • ΔH >0 and ΔS >0

  • ΔH >0 and ΔS <0


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258.

The standard Gibbs energy for the given cell reaction in kJ mol-1 at 298 K is:

Zn (s) + Cu2+ (aq) → Zn2+ (aq) + Cu (s), E° = 2V at 298 K

  • -192

  • 384

  • -384

  • 192


C.

-384

Zn (s) + Cu2+ (aq) → Zn2+ (aq) + Cu (s)

G° = -nFEcell°

        = -2 × 96000 × 2

        = -4 × 96 kJ 

        = -384 kJ


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259.

The difference between ΔH and ΔU ( ΔH- ΔU), when the combustion of one mole heptane(I) is carried out a temperature T, is equal to:

  • -3RT

  • -4RT

  • 3RT

  • 4R


260.

The correct thermodynamic conditions for  the spontaneous reaction at all temperatures is

  • ΔH> 0 and Δ S< 0
  • ΔH< 0 and ΔS > 0
  • ΔH ΔS >0
  • ΔH ΔS >0
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