A) 1.0 mole of \[{{H}_{2}}O\] is produced
B) 1.0 mole of NO will be produced
C) All the oxygen will be consumed
D) All the ammonia will be consumed
Correct Answer: C
Solution :
[c] All the oxygen will be consumed.\[As{{O}_{2}}\]will be limiting reacant. Hence, all oxygen will be consumed. As given reaction is \[\to \] \[N{{N}_{3}}+{{H}_{2}}ONH_{4}^{+}+O{{H}^{-}}\] Reaction \[N{{H}_{3}}+{{O}_{2}}\xrightarrow{{}}NO+{{H}_{2}}O\] After balancing it will turn to given equation, It means, when 4 moles of \[N{{H}_{3}}\]reaction with excess\[{{O}_{2}}\], it will form 4 moles of no. (in ratio 1:1) Limiting reagent is reactant which gets used faster and hence terminates the reaction.
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