• 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

    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 \[{{O}_{2}}\] 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.

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