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.

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Asked on June 4, 2026Chemistry

This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.

Accepted Answer · 2026-06-04T07:22:41.993Z

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 (HCl(g) and O_2(g)) and products (H_2O(g) and Cl_2(g)) are in the same physical state, which is gaseous. 6.3 To calculate the initial mass of $O_2(g ✂️ _That answer was long and got cut off. Reply continue and I'll finish it._

Accepted Answer · 2026-06-04T07:22:41.993Z

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 (HCl(g) and O_2(g)) and products (H_2O(g) and Cl_2(g)) are in the same physical state, which is gaseous. 6.3 To calculate the initial mass of $O_2(g ✂️ _That answer was long and got cut off. Reply continue and I'll finish it._

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.

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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.

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