In the reaction #N_2 + 3H_2 -> 2NH_3#, what volume of ammonia is produced when 5.0 L of Nitrogen react?
We follow the stoichiometry.........
You have written the following equation, which is stoichiometrically balanced:
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?
By signing up, you agree to our Terms of Service and Privacy Policy
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
By signing up, you agree to our Terms of Service and Privacy Policy
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.
- When heated, solid copper(II) carbonate decomposes to solid copper(II) oxide and carbon dioxide gas. What is the chemical equation (including phases) that describes this reaction?
- Elemental phosphorus gives #PH_3# and #Na^+""^(-)P(OH)_2# upon basic hydrolysis. How is the reaction formulated?
- What is conserved in a chemical reaction?
- What are subscripts used for in writing chemical equations?
- How many g of #B_2H_6# will react with 3.00 mol of #O_2#?

- 98% accuracy study help
- Covers math, physics, chemistry, biology, and more
- Step-by-step, in-depth guides
- Readily available 24/7