The fuel hydrazine, N₂H₄, can be produced by the reaction of solutions of sodium hypochlorite and ammonia. The relevant chemical equation is

If 750.0 mL of 0.806 M NaClO is mixed with excess ammonia, how many moles of hydrazine can be formed? If the final volume of the resulting solution is 1.25 L, what will be the molarity of hydrazine?

Strategy We are asked for the expected amount of a product, so this is a reaction stoichiometry problem. Because NH₃ is said to be in excess, we know that NaClO will be the limiting reactant. So we will use the given volume and concentration to find the number of moles of NaClO reacting. Then use the mole ratio from the balanced equation to find the number of moles of N₂H₄ that can be formed. Finally, we can use that number of moles and the given final volume to obtain the molarity of the N₂H₄ product.

Transcribed Image Text:

NaClO(aq) + 2 NH3(aq) → N₂H4(aq) + NaCl(aq) + H₂O(l)