Ammonia is produced from reaction with hydrogen according to equation: N(g)+3H (g)2NH (g). If 25 N; molecules react with 60 H molecules in a sealed container, which molecules will be completely consumed? How many NH, molecules are formed? Ans: H; 40 NH, molecules).
Ammonia is produced in the following reaction: N (g)+3H (g) 2NH
The balanced equation for the reaction is:
N2(g) + 3H2(g) -> 2NH3(g)
From the equation, we can see that 1 molecule of N2 reacts with 3 molecules of H2 to produce 2 molecules of NH3.
Given:
25 N2 molecules react with 60 H2 molecules.
We need to determine which molecules are completely consumed.
For every 1 molecule of N2, we need 3 molecules of H2. Therefore, the maximum number of N2 molecules that can react is 25.
Since we have 60 H2 molecules, we have more than enough to react with the available N2 molecules. Therefore, the H2 molecules are in excess and will not be completely consumed.
To find the number of NH3 molecules formed, we need to calculate the number of N2 molecules that react.
Since 1 molecule of N2 reacts with 3 molecules of H2 to form 2 molecules of NH3, the number of NH3 molecules formed will be half of the number of N2 molecules that react.
Therefore, the number of NH3 molecules formed = (25 N2 molecules / 2) = 12.5 NH3 molecules
However, we cannot have a fraction of a molecule, so we round down to the nearest whole number.
The number of NH3 molecules formed = 12 NH3 molecules.
In summary:
- The H2 molecules will be in excess and not be completely consumed.
- 12 NH3 molecules are formed.
In the given reaction, the balanced equation is:
N₂(g) + 3H₂(g) → 2NH₃(g)
Given that 25 molecules of N₂ and 60 molecules of H₂ react, we need to determine which molecules will be completely consumed and the amount of NH₃ produced.
To find out which molecules will be completely consumed, we need to identify the limiting reactant. This can be done by comparing the reactant's coefficients in the balanced equation to the amount of each reactant given.
For N₂: 25 molecules
For H₂: 60 molecules
The ratio between N₂ and H₂ in the balanced equation is 1:3. Therefore, for every 1 molecule of N₂, we need 3 molecules of H₂.
If we use up all the N₂, it would require 3 * 25 = 75 molecules of H₂. However, we only have 60 molecules of H₂, which is less than what is required for complete consumption. This means that H₂ is the limiting reactant, and N₂ will be in excess.
So, the completely consumed molecule is H₂.
To find the amount of NH₃ formed, we can use the stoichiometry from the balanced equation. Since 3 molecules of H₂ react to form 2 molecules of NH₃, we can set up a proportion:
3 H₂ : 2 NH₃
60 molecules of H₂ corresponds to x molecules of NH₃.
3/2 = 60/x
Cross-multiplying, we get:
3x = 2 * 60
3x = 120
x = 120/3
x = 40
Therefore, 40 molecules of NH₃ are formed.
In summary:
The completely consumed molecule is H₂.
The number of NH₃ molecules formed is 40.