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In the following reaction we start with ...

In the following reaction we start with 2 mol of `N_(2)` and 5 of `H_(2)` exerting a total pressure of 7 atm at a given temperature in a closed vessel when 50% of `N_(2)` is converted into `NH_(3), N_(2) + 3H_(2) to 2NH_(3)`
What will be the partial pressure of `NH_(3)` in atmosphere ?

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In the following reaction, we start with 2 mol of N_(2) and 5 mol of H_(2) exerting a total pressure of 7 atm at a given temperature is a closed vessel. When 50% of N_(2) is converted into NH_(3) . N_(2)+3H_(2)to2NH_(3) Partial pressure of NH_(3) is:

2NH_(3) to N_(2) + 3H_(2) Find moles of H_(2) produced from 4 moles of NH_(3)

Knowledge Check

  • In the following reaction, we start with 2 mol of N_2 and 5 mol of H_2 exerting a total pressure of 7 atm at a given temperature in a closed vessel. When 50% of N_2 is converted into NH_3 N_(2) + 3H_(2) to 2NH_(3) Partial pressure of NH_3 is :

    A
    2.8 atm
    B
    2 atm
    C
    3.2 atm
    D
    4 atm

  • In the folowing reaction, we start with 2 mol of N_(2) and 5 mol of H_(2) exerting a total pressure of 7 atm, at a given temperature in a closed vessel. When 50 % of N_(2) is converted into NH_(3) N_(2)+ 3H_(2) rarr 2NH_(3) Partial pressure of NH_(3) is:

    A
    2.8 atm
    B
    2 atm
    C
    3.2 atm
    D
    4 atm

  • N_(2)+3H_(2) to NH_(3)

    A
    For disproportionation reaction.
    B
    For comproportionation reaction.
    C
    For either intermolecular redox reaction or displacement reaction
    D
    For either thermal combination redox reaction or thermal decomposition redox reaction.

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