Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product formed. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that is made.
Mol N2H4 Mol N2O4 Mol N2 Mol H2O
_____ _____ 10.9 _____
Someone got happy with the instructions. Verbose I think. And you can't do this with the coefficients? Here is the first one.
You have 10.9 mols N2 if I read that table right. You want to know mols N2H4.
10.9 mol N2 x (2 mols N2H4/3 mols N2) \ 10.9 x 2/3 = ?
Or from N2 to H2O is
10.9 mols N2 x (4 mols H2O/3 mols N2) = 10.9 x (4/3) = ?
I'll bet you can do the others without any help.
bums away
To complete the table, we need to use the stoichiometry of the balanced equation to determine the appropriate number of moles of each reactant and product.
Given that the number of moles of N2 is 10.9, we can start by finding the number of moles of N2O4 required to produce that amount of N2.
From the balanced equation, we can see that the mole ratio between N2O4 and N2 is 1:3. Therefore, the number of moles of N2O4 required is:
(10.9 mol N2) / (3 mol N2O4) = 3.63 mol N2O4
Now we need to calculate the number of moles of H2O produced.
From the balanced equation, we can see that the mole ratio between N2O4 and H2O is 1:2. Therefore, the number of moles of H2O produced is:
(3.63 mol N2O4) * (4 mol H2O) / (1 mol N2O4) = 14.52 mol H2O
Finally, we can calculate the number of moles of N2H4 required.
From the balanced equation, we can see that the mole ratio between N2H4 and N2O4 is 2:1. Therefore, the number of moles of N2H4 required is:
(3.63 mol N2O4) * (2 mol N2H4) / (1 mol N2O4) = 7.26 mol N2H4
Now we can complete the table:
Mol N2H4 | Mol N2O4 | Mol N2 | Mol H2O
--------------------------------------------
7.26 | 3.63 | 10.9 | 14.52
Note: It is important to always use the stoichiometric ratios from the balanced equation to calculate the amount of reactants required or products formed.
To find the appropriate number of moles of reactants and products in the given balanced equation, we can use stoichiometry. Stoichiometry allows us to establish the quantitative relationship between the reactants and products in a chemical reaction.
Let's start by determining the number of moles of each reactant and product when 10.9 moles of N2 are formed.
Step 1: Determine the mole ratio
From the balanced equation, we can see that for every 3 moles of N2, 2 moles of N2H4 are consumed. Likewise, for every 3 moles of N2, 4 moles of H2O are formed.
Mole ratio of N2H4 to N2 = 2/3
Mole ratio of H2O to N2 = 4/3
Step 2: Calculate the number of moles of N2H4
To find the number of moles of N2H4, we can use the mole ratio:
Moles of N2H4 = Moles of N2 * Mole ratio of N2H4 to N2
Moles of N2H4 = 10.9 * (2/3)
Moles of N2H4 ≈ 7.27
Step 3: Calculate the number of moles of H2O
To find the number of moles of H2O, we can use the mole ratio:
Moles of H2O = Moles of N2 * Mole ratio of H2O to N2
Moles of H2O = 10.9 * (4/3)
Moles of H2O ≈ 14.53
Step 4: Fill in the table
Now, we can fill in the appropriate number of moles of each reactant and product in the table:
Mol N2H4 Mol N2O4 Mol N2 Mol H2O
7.27 ________ 10.9 14.53
Since we are given the number of moles of N2, we can use this information to find the number of moles of N2O4.
Step 5: Calculate the number of moles of N2O4
Using the balanced equation, we can see that the mole ratio of N2O4 to N2 is 1:3.
Moles of N2O4 = Moles of N2 * Mole ratio of N2O4 to N2
Moles of N2O4 = 10.9 * (1/3)
Moles of N2O4 ≈ 3.63
Finally, we can update the table:
Mol N2H4 Mol N2O4 Mol N2 Mol H2O
7.27 3.63 10.9 14.53
Note: The values provided here are rounded to two decimal places for simplicity.