Consider the reaction represented by the balanced equation below: 4HCl(g) + O2(g) <=> 2H2O(g) + 2Cl2(g) Initially, 1 mole of HCl (g) and an UNKNOWN mass of O2 (g) were mixed in a sealed 5 dm³ container. At 600 °C equilibrium was established and 28,40 g of Cl2 (g), was present in the container.

Here are the solutions to Question 6.

6.1
Chemical equilibrium is a state in a reversible reaction where the rate of the forward reaction is equal to the rate of the reverse reaction, and the concentrations of reactants and products remain constant.

6.2
The reaction is homogeneous because all reactants ($\text{HCl(g)}$ and $\text{O}_2\text{(g)}$) and products ($\text{H}_2\text{O(g)}$ and $\text{Cl}_2\text{(g)}$) are in the same physical state, which is gaseous.

6.3
To calculate the initial mass of $\text{O}_2\text{(g