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Question

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.


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Solution

Step-1: Calculate the value of X g of nitrogen

2NH3(g)N2(g)+3H2(g)(Ammonia)(Nitrogen)(Hydrogen)

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= 282×22.4 g of N2

448 L of ammonia gas decomposes to form= 282×22.4×448=280 g of N2

Step-2: Calculate the weight of oxygen required to react with 280 g of nitrogen to produce NO2

2O2(g)+N2(g)2NO2(g)(Oxygen)(Nitrogen)(Nitrogendioxide)

From the balanced chemical equation,

28 g of nitrogen reacts with= 64 g of oxygen

1 g of nitrogen reacts with= 6428 g of oxygen

280 g of nitrogen reacts with= 6428×280=640 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= 6.023x102332 molecules

640 g of oxygen= 6.023x102332×640=12×1024molecules

Therefore, the molecules of oxygen required to produce NO2 from X g of nitrogen are 12 ×1024 molecules.


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