In the reaction #N_2 + 3H_2 -> 2NH_3#, what volume of ammonia is produced when 5.0 L of Nitrogen react?

Answer 1

We follow the stoichiometry.........#10*L# of ammonia will result.

You have written the following equation, which is stoichiometrically balanced:

#N_2(g)+3H_2(g) rightleftharpoons 2NH_3(g)#
Given constant temperature and pressure, which we must assume, volume is proportional to the number of moles. And thus if #5.0*L# of dinitrogen react (with #15.0*L# of dihydrogen), #10.0*L# of ammonia gas will result.

The one benefit this reaction has is that the reactants are highly volatile gases and the product, ammonia, is highly soluble in water, but practically speaking, we will get nothing close to a quantitative reaction, and the reaction is an equilibrium that needs to be manipulated.

For what reason is dinitrogen reduction thought to be the most significant reaction ever carried out on Earth?

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Answer 2

To find the volume of ammonia produced, we need to use the stoichiometry of the reaction. According to the balanced equation, 1 mole of nitrogen (N₂) reacts with 3 moles of hydrogen (H₂) to produce 2 moles of ammonia (NH₃).

First, we need to calculate the moles of nitrogen present in 5.0 L:

n(N₂) = V / Vm n(N₂) = 5.0 L / 22.4 L/mol (standard molar volume at STP) n(N₂) ≈ 0.223 moles

According to the balanced equation, 1 mole of nitrogen produces 2 moles of ammonia. So, 0.223 moles of nitrogen will produce:

0.223 moles of N₂ × (2 moles of NH₃ / 1 mole of N₂) = 0.446 moles of NH₃

Now, we can calculate the volume of ammonia produced:

V(NH₃) = n(NH₃) × Vm V(NH₃) = 0.446 moles × 22.4 L/mol V(NH₃) ≈ 9.98 L

Therefore, approximately 9.98 liters of ammonia are produced when 5.0 liters of nit

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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