To determine how the system at equilibrium will be affected by removal of [tex]\( \text{H}_2 \text{O} \)[/tex], we need to apply Le Chatelier's Principle. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
The balanced chemical equation we are considering is:
[tex]\[ 2 \text{H}_2(g) + \text{O}_2(g) \leftrightarrow 2 \text{H}_2\text{O}(g) + \text{heat} \][/tex]
Here’s the step-by-step process to analyze how removal of [tex]\( \text{H}_2 \text{O} \)[/tex] will affect the equilibrium:
1. Identify the Change:
- Removal of [tex]\( \text{H}_2 \text{O} \)[/tex] means that the concentration of one of the products (water vapor) is decreased.
2. Apply Le Chatelier's Principle:
- According to Le Chatelier’s Principle, when the concentration of a product is decreased, the system will try to counteract this change by producing more of that product. This means the equilibrium will shift towards the products to increase the concentration of [tex]\( \text{H}_2\text{O} \)[/tex] again.
3. Predict the Direction of Shift:
- Since [tex]\( \text{H}_2\text{O} \)[/tex] is a product and its concentration is reduced, the system will shift right towards the production of more [tex]\( \text{H}_2\text{O} \)[/tex].
4. Conclusion:
- Removal of [tex]\( \text{H}_2\text{O} \)[/tex] will cause the equilibrium to shift towards the right, which means towards the products.
In summary, if [tex]\( \text{H}_2\text{O} \)[/tex] is removed from a system at equilibrium, the system will shift towards the products to counteract the reduction in [tex]\( \text{H}_2\text{O} \)[/tex] concentration.
