448 L of ammonia at STP on decomposition gives X g of nitrogen. How many molecules of oxygen are required to produce NO2 from X g of nitrogen.
Step-1: Calculate the value of X g of nitrogen
According to Avogadro’s law, at STP, 22.4 L of any gas weighs equal to the gram molecular weight of the substance.
The gram atomic weight of Nitrogen (N)= 14 g mol-1
The gram atomic weight of Hydrogen (H)= 1 g mol-1
Gram molecular weight of Ammonia (NH3)= 14+3(1)= 17 g mol-1
Therefore, 22.4 L of Ammonia (NH3)= 17 g of Ammonia
From the balanced chemical equation,
2× 22.4 L of ammonia gas decomposes to form= 28 g of N2
1 L of ammonia gas decomposes to form= g of N2
448 L of ammonia gas decomposes to form= g of N2
Step-2: Calculate the weight of oxygen required to react with 280 g of nitrogen to produce NO2
From the balanced chemical equation,
28 g of nitrogen reacts with= 64 g of oxygen
1 g of nitrogen reacts with= g of oxygen
280 g of nitrogen reacts with= g of oxygen
Step-3: Calculate the number of molecules of oxygen
According to the mole concept, the gram molecular weight of a substance= 6.023×1023 molecules per mole
Therefore, 32 g of oxygen= 6.023×1023 molecules
1 g of oxygen= molecules
640 g of oxygen= molecules
Therefore, the molecules of oxygen required to produce NO2 from X g of nitrogen are 12 ×1024 molecules.