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Consider the reaction:
2 NO(g) + 5 H2(g)-2 NH3(g) + 2 H2O(g)
A reaction mixture initially contains 5 moles of NO and 10 moles of H2. Without doing any calculations, determine which set of amounts best represents the mixture after the reactants have reacted as completely as possible. Explain your reasoning.
a. 1 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O
b. 0 mol NO, 1 mol H2, 5 mol NH3, 5 mol H2O
c. 3 mol NO, 5 mol H2, 2 mol NH3, 2 mol H2O
d. 0 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O

Respuesta :

After the whole feasible response of balanced equation, 1 mole of NO has remained withinside the response mixture is 1 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O.

The balanced chemical equation for

the response will be: 2 NO(g) + 5 H2(g)-2 NH3(g) + 2 H2O(g). The hydrogen required has been:

  • 2 moles NO = 5 moles hydrogen
  • five moles NO Hydrogen five 2 G x 5 moles
  • five moles NO = 5 moles Hydrogen.
  • The to be had hydrogen has been 10
  • moles.
  • 5 moles hydrogen = 2 moles NO
  • 2 10 moles hydrogen NO x 10 moles
  • 10 moles hydrogen = four moles NO.
  • The whole usage of hydrogen calls for four moles of NO. The to be had NO has been 5 moles. The final NO has been given as:
  • Remaining NO = Total - consumed
  • Remaining NO = 5-4
  • Remaining NO = 1mole
  • After the whole feasible response of the mixture, 1 mole of NO has remained withinside the response mixture.

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