1. Tardigrade
  2. Question
  3. Chemistry
  4. In the following reaction, we start with 2 moles of N2 and 5 moles of H2 exerting a total prssure of 7 aim at a given temperature in a closed vessel. When 50% of N2 s converted into NH3, partial pressure of NH3 is N2+3H2 xrightarrow[]2NH3

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Q. In the following reaction, we start with 2 moles of $ {{N}_{2}} $ and 5 moles of $ {{H}_{2}} $ exerting a total prssure of 7 aim at a given temperature in a closed vessel. When 50% of $ {{N}_{2}} $ s converted into $ N{{H}_{3}}, $ partial pressure of $ N{{H}_{3}} $ is $ {{N}_{2}}+3{{H}_{2}}\xrightarrow[{}]{{}}2N{{H}_{3}} $

JamiaJamia 2013

Solution:

$ {{N}_{2}}+3{{H}_{2}}\xrightarrow[{}]{{}}2N{{H}_{3}} $ Initial moles $ 2~~~~~~~~~~5~~~~~~~~~~~~~0 $ reacted (50% $ {{N}_{2}} $ ) $ ~1~~~~~~~~~3~~~~~~~~~~~~~~2 $ Left moles. $ 1~~~~~~~~~2~~~~~~~~~~~~~~2 $ Total number of moles of $ {{N}_{2}}{{H}_{2}} $ and $ N{{H}_{3}} $ left $ =1+2+2=5 $ Initial moles = 7 pressure at initials =7 atm pressure at equilibrium =5 atm Partial pressure of $ N{{H}_{3}}=\frac{2}{5}\times 5=2\,atm $