Respuesta :
Answer:
Option A is correct. The system is at equilibrium
Explanation:
Step 1: Data given
Kc at 1300 K = 5.00
Initial concentration of SO2 = 1.20 M
Initial concentration of O2 = 0.45 M
The concentration of SO3 = 1.80 M
When Q=K, the system is at equilibrium and there is no shift to either the left or the right.
When Q<K, there are more reactants than products. As a result, some of the reactants will become products, causing the reaction to shift to the right.
When Q>K, there are more products than reactants. To decrease the amount of products, the reaction will shift to the left and produce more reactants.
Step 2: The balanced equation
2 SO2(g) + O2(g) ⇌ 2 SO3(g)
Step 3: Calculate Q
Q = [SO3]² / [O2][SO2]²
Q = 1.80²/0.45*1.20²
Q = 5.00
Q = Kc
This means , the system is at equilibrium and there is no shift to either the left or the right.
Option A is correct.
The system is:
A) at equilibrium.
Given:
Kc at 1300 K = 5.00
Initial concentration of SO₂ = 1.20 M
Initial concentration of O₂ = 0.45 M
The concentration of SO₃ = 1.80 M
Conditions for Equilibrium constant:
1. When Q=K, the system is at equilibrium and there is no shift to either the left or the right.
2. When Q<K, there are more reactants than products. As a result, some of the reactants will become products, causing the reaction to shift forward.
3. When Q>K, there are more products than reactants. To decrease the amount of products, the reaction will shift backwards and produce more reactants.
Balanced chemical reaction:
2 SO₂(g) + O₂ (g) ⇌ 2 SO₃ (g)
Calculation for Q:
Q = [SO₃]² / [O₂][SO₂]²
Q = 1.80²/0.45*1.20²
Q = 5.00
Q = Kc
So, this is following condition 1 where the reaction is at equilibrium.
Find more information about Equilibrium here:
brainly.com/question/12858312
