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 :
\[4N{{H}_{3}}(g)+5{{O}_{2}}(g)\xrightarrow[{}]{{}}4NO(g)+6{{H}_{2}}O(\ell )\] |
\[4\,mol\,+5\,mol\,\xrightarrow[{}]{{}}4\,mol+\,6\,mol\] |
According to equation |
1 mole of O2 requires = 4/5 = 0.8 mole of \[N{{H}_{3}}\] |
While 1 mole of \[N{{H}_{3}}\] requires \[\text{=}\frac{\text{5}}{\text{4}}\text{=1}\text{.25}\] mole of \[{{O}_{2}}\] |
As there is 1 mole of \[N{{H}_{3}}\] and 1 mole of \[{{O}_{2}}\]. So, all oxygen will be consumed. |
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