A) \[1\times {{10}^{23}}\]
B) \[2\times {{10}^{23}}\]
C) \[4\times {{10}^{23}}\]
D) \[6\times {{10}^{23}}\]
Correct Answer: D
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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