Given the reaction for manufacturing hydrazine,N₂H₄,which in turn can react explosively as a rocket fuel: 2 NH₃(aq)+ NaOCl(aq)→ N₂H₄(aq)+ NaCl(aq)+ H₂O(l)
2 N₂H₄(l)+ N₂O₄(l)→ 3 N₂(g)+ 4 H₂O(g)
What volume of nitrogen gas at STP is released in the two-step process if all the N₂H₄ fuel is produced from 100.0 mL of 0.500 M NH₃?

Question

Quizplus · Accepted Answer

The first step produces 100.0 mL of 0.500 M N₂H₄. The second step produces 3 moles of N₂ for every 2 moles of N₂H₄. Therefore, the total volume of N₂ produced is:(100.0 mL)(0.500 M)(1 L/1000 mL)(3 mol N₂/2 mol N₂H₄)(22.4 L/mol N₂) = 0.840 L

Given the Reaction for Manufacturing Hydrazine,N₂H₄,which in Turn Can React