For the reaction H2(g) + I2(g) 2HI(g), Kc = 50.2 at 445ºC. If [H2] = [I2] = [HI] = 1.75  10-3 M at 445ºC, which one of these statements is true? A) The system is at equilibrium, thus no concentration changes will occur. B) The concentrations of HI and I2 will increase as the system approaches equilibrium. C) The concentration of HI will increase as the system approaches equilibrium. D) The concentrations of H2 and HI will fall as the system moves toward equilibrium. E) The concentrations of H2 and I2 will increase as the system approaches equilibrium

The reaction approaching towards equilibrium results in the increase in HI concentration. Thus, option C is correct.

The balanced chemical equation has been given as:

The equilibrium has been the condition when the concentration of reactants and products in the reaction has been equal. The given condition has equal concentration of all the compounds in the mixture.

The reactant concentration has been the sum of concentration of hydrogen and iodine.Thus, the concentration of reactants has been higher than the concentration of product HI.

Thus, on moving towards the equilibrium condition, the concentration of HI increases. Thus, option C is correct.

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C) The concentration of HI will increase as the system approaches equilibrium.

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as

K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

For the given chemical reaction:

The expression for is written as:

Thus as , the reaction will shift towards the right i.e. towards the product side.

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