Question

In Haber process
30 litre of dihydrogen is taken and 30 litre of dinitrogen is taken.
After the reaction, the product yielded was 50% of the expected product.

What will be the composition of gaseous mixture under aforesaid Condition in the end.

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Answer 1

The haber reaction is

N2 +3H2⇒2NH3

now we can see that The moles of H2 is three times that of N2.After which 2 moles of NH3 is yielded.

If we predict The Volume of NH3 it will 20 litre as the volume of Hydrogen is 30 litre so it will react only 10 litres of N2 and produce 20 litre of NH3.

so the product yielded was 1/2 of expected =10 litres of NH3.

so the composition is 5litres of N2 and 15litres of H2

Answer 2

heya answer is here..........


◇As always, start by writing the balanced chemical equation that describes this reaction

3H2(g)+N2(g)→2NH3(g)

Your first goal here is to figure out how much ammonia would be produced for a 100% yield.

To do that, use the fact that when working with constant pressure and temperature, the mole ratio that exists between the species involved in the reaction is equivalent to a volume ratio.

In other words, at 100% yield, your reaction will consume 3 liters of hydrogen gas and 1 liter of nitrogen gas and produce 2 liters of ammonia.

At this point, it should be obvious that you're dealing with a limiting reagent. Notice that in order for all the hydrogen gas to react, you need

30L H2⋅1 L N23L H2=10 L N2

Since you have more than 10 L of nitrogen gas, you can say that nitrogen is in excess, which implies that hydrogen gas is the limiting reagent here.

Now, here's where things get a little tricky. At 100%yield, the reaction will consume

30 L H2→ all the hydrogen is consumed because it acts as a limiting reagent

10 L N2

and produce

30L H2⋅2aL NH33L H

hope it helps u dear.....