Question

\\2\text{no}(\text{g}) + \text{o}_2(\text{g}) \
ightleftharpoons 2\text{no}_2(\text{g}) \quad k = 1.5 \times 10^{-10}\\

the current concentrations for the system are given below. what is the reaction quotient, \\(q\\), for the system?

\\\text{no} = 0.52\text{ m}\\
\\\text{o}_2 = 0.351\text{ m}\\
\\\text{no}_2 = 0.133\text{ m}\\

\\q = ?\\

Explanation:

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<reasoning>

Write the reaction quotient expression

Using the Reaction Quotient knowledge point
\[
Q = \frac{[\text{NO}_2]^2}{[\text{NO}]^2[\text{O}_2]}
\]

Substitute the given concentrations

Using the Reaction Quotient knowledge point
\[

$$\begin{aligned} &[\text{NO}] = 0.52\text{ M}\\ &[\text{O}_2] = 0.351\text{ M}\\ &[\text{NO}_2] = 0.133\text{ M}\\ &Q = \frac{(0.133)^2}{(0.52)^2 \times 0.351} \end{aligned}$$

\]

Calculate the final value

Using the Reaction Quotient knowledge point
\[

$$\begin{aligned} &(0.133)^2 = 0.017689\\ &(0.52)^2 = 0.2704\\ &0.2704 \times 0.351 = 0.0949104\\ &Q = \frac{0.017689}{0.0949104} \approx 0.186 \end{aligned}$$

\]
</reasoning>

<answer>
\(2\text{NO(g)} + \text{O}_2\text{(g)}
ightleftharpoons 2\text{NO}_2\text{(g)} \quad K = 1.5 \times 10^{-10}\)

The current concentrations for the system are given below. What is the reaction quotient, Q, for the system?

\([\text{NO}] = 0.52\text{ M}\)
\([\text{O}_2] = 0.351\text{ M}\)
\([\text{NO}_2] = 0.133\text{ M}\)

\(Q =\) <blank>\(0.186\)</blank>
</answer>

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Answer:

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<reasoning>

Write the reaction quotient expression

Using the Reaction Quotient knowledge point
\[
Q = \frac{[\text{NO}_2]^2}{[\text{NO}]^2[\text{O}_2]}
\]

Substitute the given concentrations

Using the Reaction Quotient knowledge point
\[

$$\begin{aligned} &[\text{NO}] = 0.52\text{ M}\\ &[\text{O}_2] = 0.351\text{ M}\\ &[\text{NO}_2] = 0.133\text{ M}\\ &Q = \frac{(0.133)^2}{(0.52)^2 \times 0.351} \end{aligned}$$

\]

Calculate the final value

Using the Reaction Quotient knowledge point
\[

$$\begin{aligned} &(0.133)^2 = 0.017689\\ &(0.52)^2 = 0.2704\\ &0.2704 \times 0.351 = 0.0949104\\ &Q = \frac{0.017689}{0.0949104} \approx 0.186 \end{aligned}$$

\]
</reasoning>

<answer>
\(2\text{NO(g)} + \text{O}_2\text{(g)}
ightleftharpoons 2\text{NO}_2\text{(g)} \quad K = 1.5 \times 10^{-10}\)

The current concentrations for the system are given below. What is the reaction quotient, Q, for the system?

\([\text{NO}] = 0.52\text{ M}\)
\([\text{O}_2] = 0.351\text{ M}\)
\([\text{NO}_2] = 0.133\text{ M}\)

\(Q =\) <blank>\(0.186\)</blank>
</answer>

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