Chapter 3, Problem 138CP

A gas contains a mixture of ${\text{NH}}_{\text{3}}\text{(}g{\text{) and N}}_{\text{2}}{\text{H}}_{\text{4}}\text{(}g\text{)}$ , both ofwhich react with ${\text{O}}_{\text{2}}\text{(}g\text{)}$ to form ${\text{NO}}_{\text{2}}\text{(}g{\text{) and H}}_{\text{2}}\text{O(}g\text{)}$ . Thegaseous mixture (with an initial mass of 61.00 g) is reactedwith 10.00 moles ${\text{O}}_{\text{2}}$ , and after the reaction iscomplete, 4.062 moles of ${\text{O}}_{\text{2}}$ remains. Calculate the masspercent of ${\text{N}}_{\text{2}}{\text{H}}_{\text{4}}\text{(}g\text{)}$ in the original gaseous mixture.