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If a mixture of 3 "mole" of H(2) and 1 "...

If a mixture of `3 "mole"` of `H_(2)` and `1 "mole"` of `N_(2)` is completely converted into `NH_(3)`, what would be the final volume at same `P` and `T`?

Text Solution

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`{:(,,N_(2),+,3H_(2),hArr,2NH_(3)),(,"Initial mole",1,,3,,0),(,"Final mole",0,,0,,2):}`
(`:'` Complete conversion)
Final volume at same `P` and `T=2`
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Knowledge Check

  • A mixture of 2 mole CO and 1 mole O_(2) in a closed vessel is ignited to convert CO into CO_(2) . Then

    A
    `Delta H=Delta E`
    B
    `DeltaH gt Delta E`
    C
    `Delta H lt Delta E`
    D
    The relationship depends upon the capacity of the vessel

  • If 1 mole of H_(2) , 2 moles of O_(2) and 3 moles of N_(2) are mixed in a vessel and total pressure was found to be 12 atm then the partial pressure exerted by N_(2) in the vessel will be

    A
    2 atm
    B
    4 atm
    C
    6 atm
    D
    12 atm

  • A mixture of 0.2 mole of N_(2) and 0.6 mole of H_(2) react to give NH_(3) according to the equation, N_(2)(g)+3H_(2)(g)iff2NH_(3)(g) at constant temperature & pressure. 40 % mole of nitrogen react at equilibrium state. Then the ratio of the final volume to the initial volume of gases are

    A
    `4 : 5`
    B
    `5 : 4`
    C
    `7 : 10`
    D
    `8 : 5`