Answered

IDNLearn.com offers a seamless experience for finding and sharing knowledge. Get timely and accurate answers to your questions from our dedicated community of experts who are here to help you.

Consider the chemical equations shown here:

[tex]\[
\begin{aligned}
2 NO_2(g) & \rightarrow 2 NO(g) + O_2(g) \\
2 NO(g) & \rightarrow N_2(g) + O_2(g) \\
N_2(g) + 2 O_2(g) & \rightarrow N_2O_4(g)
\end{aligned}
\][/tex]

What is the equation for the overall reaction obtained by adding these equations?

A. \(2 NO_2(g) \rightarrow N_2O_4(g)\)

B. \(2 N_2O_4(g) + 2 NO(g) \rightarrow 2 NO_2(g) + O_2(g)\)

C. [tex]\(N_2(g) + O_2(g) + 2 NO(g) \rightarrow N_2O_4(g)\)[/tex]

Sagot :

GinnyAnsweridn
In order to determine the overall reaction, let's add the given chemical equations and see what cancels out in the process.

The given chemical equations are:

1. \(2 \text{NO}_2(\text{g}) \rightarrow 2 \text{NO}(\text{g}) + \text{O}_2(\text{g})\)
2. \(2 \text{NO}(\text{g}) \rightarrow \text{N}_2(\text{g}) + \text{O}_2(\text{g})\)
3. \(\text{N}_2(\text{g}) + 2 \text{O}_2(\text{g}) \rightarrow \text{N}_2\text{O}_4(\text{g})\)

Let's add these equations step-by-step:

First, rewrite equations to add them:
1. \(2 \text{NO}_2(\text{g}) \rightarrow 2 \text{NO}(\text{g}) + \text{O}_2(\text{g})\)
2. \(2 \text{NO}(\text{g}) \rightarrow \text{N}_2(\text{g}) + \text{O}_2(\text{g})\)
3. \(\text{N}_2(\text{g}) + 2 \text{O}_2(\text{g}) \rightarrow \text{N}_2\text{O}_4(\text{g})\)

Now, sum the reactants and products of all three equations:

Reactants:
[tex]\[ 2 \text{NO}_2(\text{g}) + 2 \text{NO}(\text{g}) + \text{N}_2(\text{g}) + 2 \text{O}_2(\text{g}) \][/tex]

Products:
[tex]\[ 2 \text{NO}(\text{g}) + \text{O}_2(\text{g}) + \text{N}_2(\text{g}) + \text{O}_2(\text{g}) + \text{N}_2\text{O}_4(\text{g}) \][/tex]

Now, let’s look at what cancels out:
- The \(2 \text{NO}(\text{g})\) on both sides
- The \(\text{N}_2(\text{g})\) on both sides
- The \(\text{O}_2(\text{g})\) from the one in first and second reaction will contribute to cancelling out one \(\text{O}_2(\text{g})\) in the products.

This leaves us with:
- \(2 \text{NO}_2(\text{g})\)
- Production of \(\text{N}_2 \text{O}_4(\text{g})\)
- Remaining \(2 \text{O}_2(\text{g})\) cancels two \(\text{O}_2(\text{g})\) in product side

So, the overall reaction is:
[tex]\[2 \text{NO}_2(\text{g}) \rightarrow \text{N}_2\text{O}_4(\text{g})\][/tex]

This matches with the balanced overall reaction:

[tex]\[2 \text{NO}_2(\text{g}) \rightarrow \text{N}_2\text{O}_4(\text{g})\][/tex]
We value your participation in this forum. Keep exploring, asking questions, and sharing your insights with the community. Together, we can find the best solutions. IDNLearn.com provides the best answers to your questions. Thank you for visiting, and come back soon for more helpful information.