Consider the equilibrium system described by the chemical reaction below. Calculate the value of [tex]Q_p[/tex] for the initial reaction conditions:

Given:
- [tex]3.51 \, \text{atm} \, \text{CCl}_4[/tex]
- [tex]5.15 \, \text{g} \, \text{C}[/tex]
- [tex]2.09 \, \text{atm} \, \text{Cl}_2[/tex]

Chemical Reaction:
[tex]\text{CCl}_4(g) \rightleftharpoons \text{C}(s) + 2 \text{Cl}_2(g)[/tex]

Using the given data, set up the expression for [tex]Q_p[/tex]. Each reaction participant must be represented appropriately in the expression.

Once the expression is constructed, solve for [tex]Q_p[/tex].

To calculate the value of [tex]\( Q_p \)[/tex] for the equilibrium system given by the reaction:

[tex]\[ \text{CCl}_4(g) \rightleftharpoons \text{C}(s) + 2 \text{Cl}_2(g) \][/tex]

we follow these steps:

1. Identify the relevant components for the reaction quotient [tex]\( Q_p \)[/tex].

For gases, [tex]\( Q_p \)[/tex] is calculated using the partial pressures. The expression for [tex]\( Q_p \)[/tex] based on the balanced chemical equation is:

[tex]\[
Q_p = \frac{(P_{\text{Cl}_2})^2}{P_{\text{CCl}_4}}
\][/tex]

Note: Since carbon (C) is in solid form, it is not included in the expression for [tex]\( Q_p \)[/tex].

2. Substitute the given values into the expression.

- The partial pressure of [tex]\(\text{CCl}_4\)[/tex], [tex]\( P_{\text{CCl}_4} \)[/tex], is 3.51 atm.
- The partial pressure of [tex]\(\text{Cl}_2\)[/tex], [tex]\( P_{\text{Cl}_2} \)[/tex], is 2.09 atm.

Plug these values into the expression for [tex]\( Q_p \)[/tex]:

[tex]\[
Q_p = \frac{(2.09 \, \text{atm})^2}{3.51 \, \text{atm}}
\][/tex]

3. Calculate the numerical value of [tex]\( Q_p \)[/tex].

[tex]\[
Q_p = \frac{4.3681 \, \text{atm}^2}{3.51 \, \text{atm}}
\][/tex]

[tex]\[
Q_p \approx 1.244
\][/tex]

So, the value of [tex]\( Q_p \)[/tex] for the given reaction conditions is approximately 1.244.