Question

The equilibrium constant Kc for the reaction of H₂ with Cl₂ at 800 K is 64.0 H₂ (g) + Cl₂ (g) <----> 2HCl (g) If 2.34 M of H₂ is allowed to react with 2.34 M of Cl₂, what is the molar concentration of HCl at equilibrium? The equilibrium constant for the following gas phase reaction is 4.0 at a certain temperature. A reaction is carried out at this temperature starting with 1.7 mol/L of CO and 1.7 mol/L of H₂O. What will be the equilibrium concentration of H₂? CO + H₂O <----> CO₂ + H₂

Answer 1

We need to examine the stoichiometry and equilibrium constants of two chemical reactions. Firstly, the equilibrium concentration of HCl is 2.34 M in the reaction of H2 with Cl2. For the second reaction involving CO and H2O, an accurate H2 equilibrium concentration can't be determined without a complete reaction equation.

Step-by-step explanation:

The described question involves two chemical equilibrium scenarios. In the first, you have H2 reacting with Cl2 to form HCl. First, set the equilibrium constant Kc (64) equal to the concentration of products divided by the concentration of reactants, including coefficients as exponents.

Since the stoichiometry has equal moles of reactants and products, due to the Law of Mass Action, the molar concentration of HCl at equilibrium is same as initial concentration i.e., 2.34 M. The second scenario is gas phase reaction of CO with H2O to form CO2 and H2.

For this reaction, you will have to consider stoichiometry and create an ICE (Initial, Change, Equilibrium) table to find the equilibrium concentrations. Unfortunately, without the complete stoichiometric relationship or chemical equation, it's not possible to provide the exact H2 equilibrium concentration.

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