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Use Le Chatelier's Principle to account for each color change in terms of the forward or reverse direction of the reaction of Equation 17-5.

**Experiment 17 Report Sheet**

**Name:**
**Date:**

**A. A Reversible Reaction**

| Step | Solution | Color Change |
|------|----------|--------------|
| 1 | After addition of 0.25 mL of 6M NaOH | Orange |
| 2 | After addition of 6M HNO3 to above solution | Orange |
| 3 | After addition of 6M NaOH to above solution | Yellow |
| 4 | Color of CrO42- in the solution | Yellow |
| 5 | After addition of 0.3 mL of 6M HNO3 | Orange |
| 6 | After addition of 6M NaOH to above solution | Yellow |
| 7 | After addition of 6M HNO3 to above solution | Orange |

Answer :

Le Chatelier's Principle states that when a system at equilibrium is subjected to a change in temperature, pressure, or concentration of reactants or products, the system will shift in a way that minimizes the impact of the change.
In the given experiment, Equation 17-5 represents a reversible reaction. The color changes observed can be explained using Le Chatelier's Principle:
1. Orange color after the addition of 0.25 ml of 6M NaOH:
- This addition increases the concentration of a reactant (NaOH).
- According to Le Chatelier's Principle, the system will shift in the reverse direction to decrease the impact of the change.
- Therefore, the reaction will shift towards the reactants, resulting in an orange color.
2. Orange color after the addition of 6M HNO3 to the above solution:
- This addition increases the concentration of a product (HNO3).
- The system will shift in the forward direction to decrease the impact of the change.
- As a result, the reaction will shift towards the products, leading to an orange color.
3. Yellow color after the addition of NaOH to the above solution:
- This addition increases the concentration of a reactant (NaOH).
- According to Le Chatelier's Principle, the system will shift in the reverse direction to minimize the impact.
- Consequently, the reaction will shift towards the reactants, causing a yellow color.
4. Yellow color after the addition of 0.3 ml of 6M HNO3:
- This addition increases the concentration of a product (HNO3).
- The system will shift in the forward direction to counteract the change.
- Hence, the reaction will shift towards the products, resulting in a yellow color.
5. Orange color after the addition of 6M NaOH to the above solution:
- This addition increases the concentration of a reactant (NaOH).
- According to Le Chatelier's Principle, the system will shift in the reverse direction to minimize the effect.
- Therefore, the reaction will shift towards the reactants, leading to an orange color.
6. Yellow-orange color after the addition of 6M HNO3 to the above solution:
- This addition increases the concentration of a product (HNO3).
- The system will shift in the forward direction to counteract the change.
- Consequently, the reaction will shift towards the products, resulting in a yellow-orange color.
These color changes occur due to the shifts in the equilibrium position of the reaction in response to changes in reactant and product concentrations. By applying Le Chatelier's Principle, we can explain the observed color changes in terms of the forward or reverse direction of the reaction.

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