https://file.aiquickdraw.com/mathbot/file/17278920637447z2541tk.jpg

The image shows a reaction between methane (\( CH_4 \)) and chlorine (\( Cl_2 \)) to form chloroform (\( CHCl_3 \)) and hydrogen chloride (\( HCl \)):

\[
CH_4(g) + 3Cl_2(g) \rightarrow CHCl_3(g) + 3HCl(g)
\]

The problem asks to predict how the composition of the mixture will change when the temperature is raised or lowered and to determine if equilibrium shifts to the right or left. 

The reaction is **exothermic**, which means heat is produced during the reaction. According to Le Chatelier’s principle, increasing temperature will shift the equilibrium to favor the endothermic direction (the reactants side), and lowering temperature will favor the exothermic direction (the products side).

### 1. Temperature is raised:
- **Pressure of \( CH_4 \)**: Since raising the temperature shifts the equilibrium to the left (towards the reactants), the concentration of \( CH_4 \) will increase, so the pressure of \( CH_4 \) will increase.
- **Shift in equilibrium**: **To the left** (reactant side).

### 2. Temperature is lowered:
- **Pressure of \( CHCl_3 \)**: Lowering the temperature shifts the equilibrium to the right (towards the products), so the concentration and pressure of \( CHCl_3 \) will increase.
- **Shift in equilibrium**: **To the right** (product side).

Would you like further details or have any questions?

Here are five related questions you might find helpful:
1. How does pressure affect the equilibrium position in a reaction with gases?
2. What is Le Chatelier’s principle, and how is it applied in predicting equilibrium shifts?
3. How does changing the concentration of a reactant or product affect equilibrium?
4. What are the differences between exothermic and endothermic reactions in terms of energy?
5. How does the equilibrium constant \( K \) change with temperature for exothermic reactions?

**Tip:** In exothermic reactions, increasing temperature always shifts the equilibrium towards the reactants, while lowering temperature favors the products.

Methane and chlorine react to form chloroform and hydrogen chloride, as represented by the following reaction: CH4(g) + 3Cl2(g) → CHCl3(g) + 3HCl(g). The reaction is exothermic. Suppose a mixture of CH4, Cl2, CHCl3, and HCl has come to equilibrium in a closed reaction vessel. Predict what changes in composition will occur when the temperature is raised or lowered. Decide whether the equilibrium shifts to the right or left.

Learn how raising or lowering the temperature affects the equilibrium composition of an exothermic reaction between methane and chlorine. Understand the application of Le Chatelier’s Principle in predicting shifts in equilibrium.

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