Question

NUCOLIURETPrad See papr: 293 See Periodic Table constant temperature and pressure if the 1818 he nitrogen is combined with reaction proceeds tp 82.0% yield? N.(2) Lole 2N, OG)

Answer 1

Step 1: Write the balanced chemical equation

2 N₂(g) + O₂(g) ----> 2N₂O(g)

Step 2: Calculation of volume of N₂O produced

2 N₂(g) + O₂(g) ----> 2N₂O(g)

From the equation we can see that mole ration of N₂ is double as that of O₂ which means if O₂ = 178 mL used then we need

( 178× 2 ) mL = 356 mL of N₂ but given is 316 mL of N₂ So the amount of N₂O will produced according to N₂

Now from the balanced equation we can see that 2 mol of N₂ produced 2 mol of N₂O

Hence, 316 mL of N₂ will produced = 316 mL of N₂O

But since we only have 82.0% yield, that means that the volume of N2O produced will be 316 mL × ( 82 /100 ) = 259.12 mL

Hence, the volume of N₂O is produced = 259.12 mL