At Westonci.ca, we connect you with the best answers from a community of experienced and knowledgeable individuals. Experience the convenience of getting accurate answers to your questions from a dedicated community of professionals. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform.
Sagot :
Certainly! Let's walk through each question step-by-step.
### How many molecules of [tex]\( H_2 \)[/tex] are produced?
In the given balanced chemical equation:
[tex]\[ 3 Fe + 4 H_2O \rightarrow Fe_3O_4 + 4 H_2 \][/tex]
We can see that when the reaction goes to completion, 4 molecules of [tex]\( H_2 \)[/tex] are produced. So, the number of molecules of [tex]\( H_2 \)[/tex] produced is [tex]\( 4 \)[/tex].
### How many oxygen atoms are required?
From the balanced chemical equation:
[tex]\[ 3 Fe + 4 H_2O \rightarrow Fe_3O_4 + 4 H_2 \][/tex]
Each molecule of [tex]\( H_2O \)[/tex] contains 1 oxygen atom. Since 4 molecules of [tex]\( H_2O \)[/tex] are involved in the reaction, the total number of oxygen atoms required is:
[tex]\[ 4 \, \text{molecules of } H_2O \times 1 \, \text{O atom per molecule of } H_2O = 4 \text{ O atoms} \][/tex]
But we need to account for the [tex]\( O \)[/tex] atoms in [tex]\( Fe_3O_4 \)[/tex], which contains 4 oxygen atoms. Hence the total number of oxygen atoms is:
[tex]\[ 4 \times 1 \times 2 = 8 \text{ atoms} \][/tex]
### How many moles of [tex]\( Fe_3O_4 \)[/tex] are formed?
The balanced equation:
[tex]\[ 3 Fe + 4 H_2O \rightarrow Fe_3O_4 + 4 H_2 \][/tex]
indicates that 1 mole of [tex]\( Fe_3O_4 \)[/tex] is formed from the reaction of 3 moles of [tex]\( Fe \)[/tex] and 4 moles of [tex]\( H_2O \)[/tex]. Therefore, the number of moles of [tex]\( Fe_3O_4 \)[/tex] formed is [tex]\( 1 \)[/tex] mole.
### What is the mole ratio of [tex]\( Fe \)[/tex] to [tex]\( H_2O \)[/tex]?
The balanced equation shows:
[tex]\[ 3 Fe + 4 H_2O \rightarrow Fe_3O_4 + 4 H_2 \][/tex]
The mole ratio of [tex]\( Fe \)[/tex] to [tex]\( H_2O \)[/tex] is derived directly from the coefficients in the balanced equation, which is:
[tex]\[ \frac{3 \text{ moles of } Fe}{4 \text{ moles of } H_2O} = 0.75 \][/tex]
Thus, the mole ratio of [tex]\( Fe \)[/tex] to [tex]\( H_2O \)[/tex] is [tex]\( 0.75 \)[/tex].
### How many hydrogen atoms are involved in this reaction?
In the given reaction:
[tex]\[ 3 Fe + 4 H_2O \rightarrow Fe_3O_4 + 4 H_2 \][/tex]
Each [tex]\( H_2O \)[/tex] molecule contains 2 hydrogen atoms. Hence, 4 molecules of [tex]\( H_2O \)[/tex] contain:
[tex]\[ 4 \times 2 = 8 \text{ H atoms} \][/tex]
Each [tex]\( H_2 \)[/tex] molecule also contains 2 hydrogen atoms. Therefore, 4 molecules of [tex]\( H_2 \)[/tex] contain:
[tex]\[ 4 \times 2 = 8 \text{ H atoms} \][/tex]
But since we consider both the hydrogen atoms in reactants and products, the total is:
[tex]\[ 4 \text{ molecules of } H_2O \times 2 \, \text{H atoms per molecule} + 4 \text{ H molecules from product} \times 2 \, \text{H atoms per molecule} = 16 \text{ atoms} \][/tex]
So, to summarize the answers:
1. The number of molecules of [tex]\( H_2 \)[/tex] produced is [tex]\( 4 \)[/tex].
2. The number of oxygen atoms required is [tex]\( 8 \)[/tex].
3. The number of moles of [tex]\( Fe_3O_4 \)[/tex] formed is [tex]\( 1 \)[/tex].
4. The mole ratio of [tex]\( Fe \)[/tex] to [tex]\( H_2O \)[/tex] is [tex]\( 0.75 \)[/tex].
5. The number of hydrogen atoms involved in this reaction is [tex]\( 16 \)[/tex].
### How many molecules of [tex]\( H_2 \)[/tex] are produced?
In the given balanced chemical equation:
[tex]\[ 3 Fe + 4 H_2O \rightarrow Fe_3O_4 + 4 H_2 \][/tex]
We can see that when the reaction goes to completion, 4 molecules of [tex]\( H_2 \)[/tex] are produced. So, the number of molecules of [tex]\( H_2 \)[/tex] produced is [tex]\( 4 \)[/tex].
### How many oxygen atoms are required?
From the balanced chemical equation:
[tex]\[ 3 Fe + 4 H_2O \rightarrow Fe_3O_4 + 4 H_2 \][/tex]
Each molecule of [tex]\( H_2O \)[/tex] contains 1 oxygen atom. Since 4 molecules of [tex]\( H_2O \)[/tex] are involved in the reaction, the total number of oxygen atoms required is:
[tex]\[ 4 \, \text{molecules of } H_2O \times 1 \, \text{O atom per molecule of } H_2O = 4 \text{ O atoms} \][/tex]
But we need to account for the [tex]\( O \)[/tex] atoms in [tex]\( Fe_3O_4 \)[/tex], which contains 4 oxygen atoms. Hence the total number of oxygen atoms is:
[tex]\[ 4 \times 1 \times 2 = 8 \text{ atoms} \][/tex]
### How many moles of [tex]\( Fe_3O_4 \)[/tex] are formed?
The balanced equation:
[tex]\[ 3 Fe + 4 H_2O \rightarrow Fe_3O_4 + 4 H_2 \][/tex]
indicates that 1 mole of [tex]\( Fe_3O_4 \)[/tex] is formed from the reaction of 3 moles of [tex]\( Fe \)[/tex] and 4 moles of [tex]\( H_2O \)[/tex]. Therefore, the number of moles of [tex]\( Fe_3O_4 \)[/tex] formed is [tex]\( 1 \)[/tex] mole.
### What is the mole ratio of [tex]\( Fe \)[/tex] to [tex]\( H_2O \)[/tex]?
The balanced equation shows:
[tex]\[ 3 Fe + 4 H_2O \rightarrow Fe_3O_4 + 4 H_2 \][/tex]
The mole ratio of [tex]\( Fe \)[/tex] to [tex]\( H_2O \)[/tex] is derived directly from the coefficients in the balanced equation, which is:
[tex]\[ \frac{3 \text{ moles of } Fe}{4 \text{ moles of } H_2O} = 0.75 \][/tex]
Thus, the mole ratio of [tex]\( Fe \)[/tex] to [tex]\( H_2O \)[/tex] is [tex]\( 0.75 \)[/tex].
### How many hydrogen atoms are involved in this reaction?
In the given reaction:
[tex]\[ 3 Fe + 4 H_2O \rightarrow Fe_3O_4 + 4 H_2 \][/tex]
Each [tex]\( H_2O \)[/tex] molecule contains 2 hydrogen atoms. Hence, 4 molecules of [tex]\( H_2O \)[/tex] contain:
[tex]\[ 4 \times 2 = 8 \text{ H atoms} \][/tex]
Each [tex]\( H_2 \)[/tex] molecule also contains 2 hydrogen atoms. Therefore, 4 molecules of [tex]\( H_2 \)[/tex] contain:
[tex]\[ 4 \times 2 = 8 \text{ H atoms} \][/tex]
But since we consider both the hydrogen atoms in reactants and products, the total is:
[tex]\[ 4 \text{ molecules of } H_2O \times 2 \, \text{H atoms per molecule} + 4 \text{ H molecules from product} \times 2 \, \text{H atoms per molecule} = 16 \text{ atoms} \][/tex]
So, to summarize the answers:
1. The number of molecules of [tex]\( H_2 \)[/tex] produced is [tex]\( 4 \)[/tex].
2. The number of oxygen atoms required is [tex]\( 8 \)[/tex].
3. The number of moles of [tex]\( Fe_3O_4 \)[/tex] formed is [tex]\( 1 \)[/tex].
4. The mole ratio of [tex]\( Fe \)[/tex] to [tex]\( H_2O \)[/tex] is [tex]\( 0.75 \)[/tex].
5. The number of hydrogen atoms involved in this reaction is [tex]\( 16 \)[/tex].
Thank you for visiting. Our goal is to provide the most accurate answers for all your informational needs. Come back soon. We hope you found this helpful. Feel free to come back anytime for more accurate answers and updated information. Westonci.ca is your trusted source for answers. Visit us again to find more information on diverse topics.
