profile-img
Anuradha bhogaonkar Asked a Question
May 11, 2020 11:49 ampts 30 pts
The following sequence of reaction occurs in commercial production of aqueous nitric acid. 4NH,(g)+50, (g) 4NO(g) + 6H,O0) AH=-904kJ.1) 3NO, (g)+H,O0)2HNO, (aq)+NO(g) AH=-140kJ.) Determine the total heat liberated (in kJ/mol) at constant pressure for the production of exactly 1 mole of aqueous nitric acid from NH3 by this process. 2NO(g)+0,(g) 2NO, (g) AH=-112kJ ..(2) a.(A) 986 b.(B) 493 c. (C) 246.5 d.(D) None of these
  • 1 Answer(s)
  • 0 Likes
  • 4 Comments
  • Shares
  • Dinesh khalmaniya thankyou
    yeh option b is correct.. here negative charge showing that it is exothermic reaction
    Likes(1) Reply(1)
    Anuradha bhogaonkar
    yes sir
  • Anuradha bhogaonkar
    ans is 493
    Likes(0) Reply(0)
  • Dinesh khalmaniya
    Multiply the first equation by 3, the second by 6, and the third by 4: 12 NH3(g) + 15 O2(g) → 12 NO(g) + 18 H2O(l) ΔH = −2721 kJ 12 NO(g) + 6 O2(g) → 12 NO2(g) ΔH = −678 kJ 12 ...
    Show more
    Likes(0) Reply(0)
  • Suresh khokhar
    follow the instructions
    • cropped6330520203082799596.jpg
    Likes(0) Reply(0)