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
2 _____ _____ _____
_____ 9 _____ _____
_____ _____ _____ 10
4.5 _____ _____ _____
_____ 3.6 _____ ____
_____ _____ 14.5 _____

Spacing makes this a little hard to read but the first row is

2 mols N2H4 will use 1 mol N2O4 to produce 3 mols N2 and 4 mols H2O. You just follow the coefficients in the balanced equation.

2,4,6,8

To complete the table, we need to use the stoichiometry of the balanced equation, which tells us the molar ratio between the reactants and products.

Let's start with the first row:
Mol N2H4: 2
Since N2H4 is given, we can use the stoichiometry to find the moles of N2O4, N2, and H2O.

2N2H4(g) + N2O4(g) → 3N2(g) + 4H2O(g)

From the equation, we know that the molar ratio between N2H4 and N2O4 is 2:1. Therefore, the moles of N2O4 would be half of the moles of N2H4.

Mol N2H4: 2
Mol N2O4: 1 (2/2)
Mol N2: 3 (3/2 * 2)
Mol H2O: 4 (4/2 * 2)

Now let's move on to the second row:
Mol N2O4: 9
Using the stoichiometry, we can find the corresponding moles of N2H4, N2, and H2O.

Mol N2O4: 9
Since the molar ratio between N2O4 and N2H4 is 1:2, the moles of N2H4 would be double the moles of N2O4.

Mol N2O4: 9
Mol N2H4: 18 (9*2)
Mol N2: 27 (9*3)
Mol H2O: 36 (9*4)

Next, we move to the third row:
Mol H2O: 10
From the balanced equation, we can determine the moles of N2H4, N2O4, and N2.

Mol H2O: 10
The molar ratio between H2O and N2O4 is 4:1, so the moles of N2O4 would be a quarter of the moles of H2O.

Mol H2O: 10
Mol N2O4: 2.5 (10/4)
Mol N2: 7.5 (2.5*3)
Mol N2H4: 5 (2.5*2)

Now, let's look at the fourth row:
Mol N2H4: 4.5
Using stoichiometry, we can calculate the moles of N2O4, N2, and H2O.

Mol N2H4: 4.5
Since the molar ratio between N2H4 and N2O4 is 2:1, the moles of N2O4 would be half the moles of N2H4.

Mol N2H4: 4.5
Mol N2O4: 2.25 (4.5/2)
Mol N2: 6.75 (2.25*3)
Mol H2O: 9 (2.25*4)

Lastly, let's consider the fifth row:
Mol N2O4: 3.6
Using the stoichiometry, we can find the moles of N2H4, N2, and H2O.

Mol N2O4: 3.6
Since the molar ratio between N2O4 and N2H4 is 1:2, the moles of N2H4 would be double the moles of N2O4.

Mol N2O4: 3.6
Mol N2H4: 7.2 (3.6*2)
Mol N2: 10.8 (3.6*3)
Mol H2O: 14.4 (3.6*4)

Finally, let's look at the last row:
Mol N2: 14.5
From the balanced equation, we can determine the moles of N2H4, N2O4, and H2O.

Mol N2: 14.5
Since the molar ratio between N2 and N2H4 is 3:2, the moles of N2H4 would be two-thirds of the moles of N2.

Mol N2: 14.5
Mol N2H4: 9.67 (14.5*2/3)
Mol N2O4: 4.83 (9.67/2)
Mol H2O: 19.33 (4.83*4)

Therefore, the completed table is as follows:

Mol N2H4 Mol N2O4 Mol N2 Mol H2O
2 1 3 4
18 9 27 36
5 2.5 7.5 10
4.5 2.25 6.75 9
7.2 3.6 10.8 14.4
9.67 4.83 14.5 19.33

To complete the table, we need to use the stoichiometry of the balanced equation to determine the number of moles of each substance involved in the reaction.

Let's go step by step:

1) Mol N2H4 = 2
Based on the balanced equation, we have 2 moles of N2H4. From the stoichiometry, we can see that for every 2 moles of N2H4, 1 mole of N2O4 is required. Therefore, for 2 moles of N2H4, we need 1 mole of N2O4. Additionally, for every 2 moles of N2H4, we obtain 3 moles of N2 and 4 moles of H2O. So, for the given 2 moles of N2H4, we have:

Mol N2O4 = 1
Mol N2 = 3
Mol H2O = 4

2) Mol N2O4 = 9
We are given 9 moles of N2O4. According to the stoichiometry, for every 1 mole of N2O4, we need 2 moles of N2H4. Therefore, for 9 moles of N2O4, we will require 2 times that, which is 18 moles of N2H4. Additionally, we can determine the amount of N2 and H2O formed. For 9 moles of N2O4, we have:

Mol N2H4 = 18
Mol N2 = 27
Mol H2O = 36

3) Mol H2O = 10
Given 10 moles of H2O, we can use the stoichiometry to find the corresponding amounts of N2H4, N2O4, and N2. Looking at the balanced equation, we see that for every 4 moles of H2O formed, we need 2 moles of N2H4. Therefore, for 10 moles of H2O, we will require half of that, which is 5 moles of N2H4. Additionally, for every 4 moles of H2O, 1 mole of N2O4 is needed. So, for 10 moles of H2O:

Mol N2H4 = 5
Mol N2O4 = 2.5
Mol N2 = 7.5

4) Mol N2H4 = 4.5
For 4.5 moles of N2H4, we can determine the corresponding amounts of N2O4, N2, and H2O. From the balanced equation, we know that for every 2 moles of N2H4, we need 1 mole of N2O4. Therefore, for 4.5 moles of N2H4, we need half that amount, which is 2.25 moles of N2O4. Moreover, for every 2 moles of N2H4, we obtain 3 moles of N2 and 4 moles of H2O. Thus, for 4.5 moles of N2H4:

Mol N2O4 = 2.25
Mol N2 = 6.75
Mol H2O = 9

5) Mol N2O4 = 3.6
Given 3.6 moles of N2O4, we can use the stoichiometry to determine the corresponding amounts of N2H4, N2, and H2O. According to the balanced equation, for every 1 mole of N2O4, we require 2 moles of N2H4. Hence, for 3.6 moles of N2O4, we need twice that amount, which is 7.2 moles of N2H4. Additionally, for every 1 mole of N2O4, we obtain 3 moles of N2 and 4 moles of H2O. Therefore, for 3.6 moles of N2O4:

Mol N2H4 = 7.2
Mol N2 = 10.8
Mol H2O = 14.4

6) Mol N2 = 14.5
For 14.5 moles of N2, we can use the stoichiometry to determine the corresponding amounts of N2H4, N2O4, and H2O. From the balanced equation, we observe that for every 3 moles of N2, we require 2 moles of N2H4. Consequently, for 14.5 moles of N2, we need 2/3 times that amount, which is 9.67 moles of N2H4. Moreover, for every 3 moles of N2, we obtain 4 moles of H2O. Thus, for 14.5 moles of N2:

Mol N2H4 = 9.67
Mol N2O4 = 6.11
Mol H2O = 19.33

I hope this helps you complete the table for the given amounts of reactants and products!