Consider the chemical equation in equilibrium.
2 answers:
Answer: A. The equilibrium will shift to the left to favor the reverse reaction.
Explanation:
Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.
This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.
For the given equation:
If the pressure is increased, the volume will decrease according to Boyle's Law. Now, according to the Le-Chatelier's principle, the equilibrium will shift in the direction where decrease in pressure is taking place. As the number of moles of gas molecules is lesser at the reactant side. So, the equilibrium will shift in the left direction to favor the formation of reactants in reverse reaction.
You might be interested in
Answer:
Explanation:
This is a typical double replacement or double decomposition reaction. In this kind of reaction, it involves the combination of ionic compounds which exchange their partners to form new compounds. Typical of these reaction is the formation of precipitates which are insoluble compounds.
The reaction equation is shown below:
AgNO₃ + K₂SO₄
→ 2KNO₃
+ AgSO₄
)
From the rule of solubility:
- All trioxonitrate(v) salts are soluble
- Salts of silver sulfates are slightly soluble. This will form the precipitate in the solution.
We can write the ionic equation as:
Ag⁺ + NO₃⁻
+ 2K⁺
+ SO₄²⁻
→ AgSO₄
+ 2K⁺ + NO₃⁻
The spectator ions or non-reactive ions are those ions that appears on both sides of the equation. These ions are the potassium and trioxonitrate ions. We cancel them out to give the net ionic equation of the reaction:
Ag⁺ + SO₄²⁻
→ AgSO₄