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Ruchi. Group Title

Calculate the mass of ammonia produced of 2g N2 reacts with 1g H2.

  • 2 years ago
  • 2 years ago

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  1. Ruchi. Group Title
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    @TheMind @ujjwal @ajprincess

    • 2 years ago
  2. UnkleRhaukus Group Title
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    have you got an equation for the reaction

    • 2 years ago
  3. Ruchi. Group Title
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    no

    • 2 years ago
  4. UnkleRhaukus Group Title
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    do you know the for mula for ammonia?

    • 2 years ago
  5. UnkleRhaukus Group Title
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    is it NH_3 ?

    • 2 years ago
  6. Ruchi. Group Title
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    nh3

    • 2 years ago
  7. UnkleRhaukus Group Title
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    so far we have \[N_2+H_2 \longrightarrow NH_3\] right?

    • 2 years ago
  8. Ruchi. Group Title
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    @@@UnkleRhaukus

    • 2 years ago
  9. UnkleRhaukus Group Title
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    can you balance the equation for number of H and N on each side?

    • 2 years ago
  10. Ruchi. Group Title
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    UR EQ IS NT APPEARING

    • 2 years ago
  11. UnkleRhaukus Group Title
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    oh,

    • 2 years ago
  12. UnkleRhaukus Group Title
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    N_2 + H_2 ⟶ NH_3

    • 2 years ago
  13. UnkleRhaukus Group Title
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    so to make the product we need thee time as much H as N

    • 2 years ago
  14. ujjwal Group Title
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    \[N_2+3H_2\rightarrow2NH_3\] You get no of moles required from this equation! Convert them in terms of weight.. Find limiting reactant (the reactant whose quantity is less than required)! limiting reactant will determine the amount of product formed!

    • 2 years ago
  15. bthemesandtricks Group Title
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    Is this always the case??

    • 2 years ago
  16. Ruchi. Group Title
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    ITS AGAIN APPEARING MATHS PROCCESING ERROR

    • 2 years ago
  17. mayankdevnani Group Title
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    i think ujjwal is right

    • 2 years ago
  18. mayankdevnani Group Title
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    N2 + 3H2 ---> 2NH3

    • 2 years ago
  19. mayankdevnani Group Title
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    So the moles are: For nitrogen, 28g/28g/mol = 1.0 mole N2 For hydrogen 25g/2g/mole = 12.5 moles @ujjwal right...

    • 2 years ago
  20. UnkleRhaukus Group Title
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    which is the limiting reagent ?

    • 2 years ago
  21. mayankdevnani Group Title
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    Obviously, hydrogen is in excess and nitrogen is the limiting reagant

    • 2 years ago
  22. mayankdevnani Group Title
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    @UnkleRhaukus

    • 2 years ago
  23. UnkleRhaukus Group Title
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    so according to the balanced equation the theoretical yield will be 2 moles of NH_3

    • 2 years ago
  24. ujjwal Group Title
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    yep! 2 mol of NH3 will be yielded!

    • 2 years ago
  25. UnkleRhaukus Group Title
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    the molar mass of ammonia is (1x14+3x1) g/mol

    • 2 years ago
  26. UnkleRhaukus Group Title
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    can you finish @Ruchi. ?

    • 2 years ago
  27. Ruchi. Group Title
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    @mayank i'm nt getting u properly

    • 2 years ago
  28. Ruchi. Group Title
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    @taylorrrr @ajprincess @imron07 @TheMind @Vikt0r hlp me out

    • 2 years ago
  29. ajprincess Group Title
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    Where are u stuck @Ruchi.?

    • 2 years ago
  30. ajprincess Group Title
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    Did u understand the part where the moles are calculated?

    • 2 years ago
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