Please wait...

Thermodynamics Test - 37
Result
Thermodynamics Test - 37

  • /

    Score

  • -

    Rank
Time Taken: -
  • Question 1/10
    4 / -1
    Consider the following reactions at 1100°C
    (I) 2C + O2 → 2CO, ∆G° = - 460 kJ mol-1
    (II) 2Zn + O2 → 2 ZnO, ∆G° = - 360 kJ mol-1
    Based on these, select correct alternate.
    Solutions

  • Question 2/10
    4 / -1
    For which reaction change of entropy will be positive ?
  • Question 3/10
    4 / -1
    The value of log Kc for a reaction
    A ⇌ B is (Given, ∆r H° 298 K = - 54.07 kJ mol-1 , ∆r S ° 298 K =10 JK-1 mol-1 and R = 8.314 JK-1 mol-1 2.303 × 8.314 × 298 = 5705)
  • Question 4/10
    4 / -1
    Enthalpy is equal to
  • Question 5/10
    4 / -1
    In an irreversible process taking place at constant T and p and in which only pressure-volume work is being done, the change in Gibbs free energy (dG) and change in entropy (dS ), satisfy the criteria.
  • Question 6/10
    4 / -1
    For the reaction at 298 K
    A(g) + B(g) ⇌ C(g) + D(g)
    ∆H° = - 29.8 kcal , ∆S° = - 0.100 kcal K-1
    What is the value of ∆G° ?
  • Question 7/10
    4 / -1
    The direct conversion of A to B is difficult, hence it is carried out by the following shown path

    Solutions

  • Question 8/10
    4 / -1
    The internal energy of one mole of a monoatomic gas is
    Solutions

  • Question 9/10
    4 / -1
    The correct relationship between ∆H and ∆E for an ideal gas at constant temperature is
  • Question 10/10
    4 / -1
    You are given the following two reactions:
    (i)CH4(g) + 202(g) → CO2 (g) + 2H2O(g), ∆H = - 890.4 kJ.
    (ii)2HgO(s) → 2Hg(l) + O2(g) – 181.6 kJ
    Which one of the following statements is correct
User Profile
-

Correct (-)

Wrong (-)

Skipped (-)

  • 1
  • 2
  • 3
  • 4
  • 5
  • 6
  • 7
  • 8
  • 9
  • 10
Get latest Exam Updates
& Study Material Alerts!
No, Thanks
Click on Allow to receive notifications
×
Open Now