At Westonci.ca, we provide clear, reliable answers to all your questions. Join our vibrant community and get the solutions you need. Our platform provides a seamless experience for finding reliable answers from a knowledgeable network of professionals. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform.
Sagot :
To solve the problem of finding the overall equation for the reaction that produces [tex]\( \text{CCl}_4 \)[/tex] and [tex]\( \text{HCl} \)[/tex] from [tex]\( \text{CH}_4 \)[/tex] and [tex]\( \text{Cl}_2 \)[/tex], follow these steps:
### Step-by-Step Solution:
Given Chemical Equations:
1. [tex]\( \text{C} (s) + 2 \text{H}_2 (g) \rightarrow \text{CH}_4 (g) \)[/tex]
2. [tex]\( \text{C} (s) + 2 \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) \)[/tex]
3. [tex]\( \text{H}_2 (g) + \text{Cl}_2 (g) \rightarrow 2 \text{HCl} (g) \)[/tex]
We need to derive an overall balanced equation that produces [tex]\( \text{CCl}_4 \)[/tex] and [tex]\( \text{HCl} \)[/tex] from [tex]\( \text{CH}_4 \)[/tex] and [tex]\( \text{Cl}_2 \)[/tex].
### Step 1: Writing the Target Reaction
Let's consider the desired reaction:
[tex]\[ \text{CH}_4 (g) + \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) + \text{HCl} (g) \][/tex]
### Step 2: Balancing the Equation
In this reaction, we need both carbon and chlorine atoms to balance out on both sides, and we should also ensure the hydrogen atoms are equally balanced.
- Carbon Balance: One C atom on both sides (from [tex]\( \text{CH}_4 \)[/tex] and [tex]\( \text{CCl}_4 \)[/tex]).
- Chlorine Balance: Start with 4 chlorine atoms from [tex]\( \text{Cl}_2 \)[/tex] to match the [tex]\( \text{CCl}_4 \)[/tex] on the product side.
- Hydrogen Balance: [tex]\( \text{CH}_4 \)[/tex] has 4 hydrogen atoms, which will form 4 molecules of [tex]\( \text{HCl} \)[/tex] since each [tex]\( \text{HCl} \)[/tex] contains 1 hydrogen atom.
### Step 3: Adjusting Coefficients
The equation must be balanced such that the number of each type of atom on the reactants side equals the number of those atoms on the products side.
[tex]\[ \text{CH}_4 (g) + 4 \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) + 4 \text{HCl} (g) \][/tex]
- Carbon atoms: 1 on both sides.
- Hydrogen atoms: 4 on both sides.
- Chlorine atoms: 8 on both sides (each [tex]\( \text{Cl}_2 \)[/tex] provides 2 atoms, so 4 [tex]\( \text{Cl}_2 \)[/tex] contribute 8 chlorine atoms, which are distributed as 4 in [tex]\( \text{CCl}_4 \)[/tex] and 4 in [tex]\( \text{HCl} \)[/tex]).
### Conclusion:
The overall balanced equation for the reaction that produces [tex]\( \text{CCl}_4 \)[/tex] and [tex]\( \text{HCl} \)[/tex] from [tex]\( \text{CH}_4 \)[/tex] and [tex]\( \text {Cl}_2 \)[/tex] is:
[tex]\[ \text{CH}_4 (g) + 4 \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) + 4 \text{HCl} (g) \][/tex]
So, the balanced chemical equation is:
[tex]\[ \boxed{\text{CH}_4 (g) + 4 \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) + 4 \text{HCl} (g)} \][/tex]
### Step-by-Step Solution:
Given Chemical Equations:
1. [tex]\( \text{C} (s) + 2 \text{H}_2 (g) \rightarrow \text{CH}_4 (g) \)[/tex]
2. [tex]\( \text{C} (s) + 2 \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) \)[/tex]
3. [tex]\( \text{H}_2 (g) + \text{Cl}_2 (g) \rightarrow 2 \text{HCl} (g) \)[/tex]
We need to derive an overall balanced equation that produces [tex]\( \text{CCl}_4 \)[/tex] and [tex]\( \text{HCl} \)[/tex] from [tex]\( \text{CH}_4 \)[/tex] and [tex]\( \text{Cl}_2 \)[/tex].
### Step 1: Writing the Target Reaction
Let's consider the desired reaction:
[tex]\[ \text{CH}_4 (g) + \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) + \text{HCl} (g) \][/tex]
### Step 2: Balancing the Equation
In this reaction, we need both carbon and chlorine atoms to balance out on both sides, and we should also ensure the hydrogen atoms are equally balanced.
- Carbon Balance: One C atom on both sides (from [tex]\( \text{CH}_4 \)[/tex] and [tex]\( \text{CCl}_4 \)[/tex]).
- Chlorine Balance: Start with 4 chlorine atoms from [tex]\( \text{Cl}_2 \)[/tex] to match the [tex]\( \text{CCl}_4 \)[/tex] on the product side.
- Hydrogen Balance: [tex]\( \text{CH}_4 \)[/tex] has 4 hydrogen atoms, which will form 4 molecules of [tex]\( \text{HCl} \)[/tex] since each [tex]\( \text{HCl} \)[/tex] contains 1 hydrogen atom.
### Step 3: Adjusting Coefficients
The equation must be balanced such that the number of each type of atom on the reactants side equals the number of those atoms on the products side.
[tex]\[ \text{CH}_4 (g) + 4 \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) + 4 \text{HCl} (g) \][/tex]
- Carbon atoms: 1 on both sides.
- Hydrogen atoms: 4 on both sides.
- Chlorine atoms: 8 on both sides (each [tex]\( \text{Cl}_2 \)[/tex] provides 2 atoms, so 4 [tex]\( \text{Cl}_2 \)[/tex] contribute 8 chlorine atoms, which are distributed as 4 in [tex]\( \text{CCl}_4 \)[/tex] and 4 in [tex]\( \text{HCl} \)[/tex]).
### Conclusion:
The overall balanced equation for the reaction that produces [tex]\( \text{CCl}_4 \)[/tex] and [tex]\( \text{HCl} \)[/tex] from [tex]\( \text{CH}_4 \)[/tex] and [tex]\( \text {Cl}_2 \)[/tex] is:
[tex]\[ \text{CH}_4 (g) + 4 \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) + 4 \text{HCl} (g) \][/tex]
So, the balanced chemical equation is:
[tex]\[ \boxed{\text{CH}_4 (g) + 4 \text{Cl}_2 (g) \rightarrow \text{CCl}_4 (g) + 4 \text{HCl} (g)} \][/tex]
We appreciate your visit. Our platform is always here to offer accurate and reliable answers. Return anytime. We appreciate your time. Please revisit us for more reliable answers to any questions you may have. Get the answers you need at Westonci.ca. Stay informed with our latest expert advice.