• # question_answer                 In the reaction                                                  $4N{{H}_{3}}(g)+5{{O}_{2}}(g)\to 4NO(g)\,+6{{H}_{2}}O(l)$                 when 1 mole of ammonia and 1 mole of ${{O}_{2}}$ are made to react to completion then :      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

$4N{{H}_{3}}(g)+5{{O}_{2}}(g)\xrightarrow[{}]{{}}4NO(g)+6{{H}_{2}}O(\ell )$                 $4\,mol\,+5\,mol\,\xrightarrow[{}]{{}}4\,mol+\,6\,mol$                 According to equation                 1 mole of ${{O}_{2}}$ requires = 4/5 = 0.8 mole of $N{{H}_{3}}$                 While 1 mole of $N{{H}_{3}}$ requires                 $=\frac{5}{4}=1.25\,mole\,of\,{{O}_{2}}$                 As there is 1 mole of $N{{H}_{3}}$ and 1 mole of ${{O}_{2}}$. So, all oxygen will be consumed.