IDNLearn.com offers a user-friendly platform for finding and sharing knowledge. Get step-by-step guidance for all your technical questions from our dedicated community members.

Consider the following intermediate chemical equations:

[tex]\[
\begin{array}{l}
2 H_2(g) + O_2(g) \rightarrow 2 H_2O(l) \\
H_2(g) + F_2(g) \rightarrow 2 HF(g)
\end{array}
\][/tex]

In the final chemical equation, [tex]$HF$[/tex] and [tex]$O_2$[/tex] are the products that are formed through the reaction between [tex]$H_2O$[/tex] and [tex]$F_2$[/tex]. Before you can add these intermediate chemical equations, you need to alter them by:

A. Multiplying the second equation by 2 and reversing the first equation.
B. Multiplying the first equation by 2 and reversing it.
C. Multiplying the first equation by [tex]\( \frac{1}{2} \)[/tex] and reversing the second equation.
D. Multiplying the second equation by 2 and reversing it.


Sagot :

Let's outline a detailed, step-by-step solution to transform and combine these intermediate chemical equations according to the given instructions:

1. Initial Equations:
- Equation 1: [tex]\( 2 H_2(g) + O_2(g) \rightarrow 2 H_2O(l) \)[/tex]
- Equation 2: [tex]\( H_2(g) + F_2(g) \rightarrow 2 HF(g) \)[/tex]

2. Alter Equation 2 by Multiplying It by 2:
- Original Equation 2: [tex]\( H_2(g) + F_2(g) \rightarrow 2 HF(g) \)[/tex]
- Multiply all coefficients by 2:
[tex]\[ 2[H_2(g) + F_2(g)] \rightarrow 4 HF(g) \][/tex]
- The simplified form is:
[tex]\[ 2 H_2(g) + 2 F_2(g) \rightarrow 4 HF(g) \][/tex]

3. Reverse Equation 1:
- Original Equation 1: [tex]\( 2 H_2(g) + O_2(g) \rightarrow 2 H_2O(l) \)[/tex]
- Reverse the equation:
[tex]\[ 2 H_2O(l) \rightarrow 2 H_2(g) + O_2(g) \][/tex]

4. Resulting Altered Equations:
- Altered Equation 1 (Reversed): [tex]\( 2 H_2O(l) \rightarrow 2 H_2(g) + O_2(g) \)[/tex]
- Altered Equation 2 (Multiplied by 2): [tex]\( 2 H_2(g) + 2 F_2(g) \rightarrow 4 HF(g) \)[/tex]

Therefore, based on the given instructions, we have:
[tex]\[ 2 H_2O(l) \rightarrow 2 H_2(g) + O_2(g) \][/tex]
[tex]\[ 2 H_2(g) + 2 F_2(g) \rightarrow 4 HF(g) \][/tex]

The final forms of the altered equations are:
- Equation 1: [tex]\( 2 H_2O(l) \rightarrow 2 H_2(g) + O_2(g) \)[/tex]
- Equation 2: [tex]\( 2 H_2(g) + 2 F_2(g) \rightarrow 4 HF(g) \)[/tex]

These are the intermediates needed to form the desired chemical reaction with [tex]\(HF\)[/tex] and [tex]\(O_2\)[/tex] as the products using [tex]\(H_2O\)[/tex] and [tex]\(F_2\)[/tex].
We appreciate your participation in this forum. Keep exploring, asking questions, and sharing your insights with the community. Together, we can find the best solutions. Thank you for trusting IDNLearn.com. We’re dedicated to providing accurate answers, so visit us again for more solutions.