Question

How would you work out part d of this question? The textbook answer is attached below, but I'm not sure how they got to the answer. Also for part b of the question, would it still be correct if I combined 2H+ and 2I- together and wrote 2HI instead?

Answer 1

To solve part d, calculate the equilibrium constant using the provided equilibrium concentrations with an ICE chart. For part b, 2H+ and 2I- should not be combined as 2HI in a dissociation reaction, as they are individual ions.

Step-by-step explanation:

To work out part d of the question involving the reaction H2(g) + I2(g) ⇒ 2HI(g), you must use the equilibrium concentrations given in the question to calculate the equilibrium constant (K). An ICE (Initial, Change, Equilibrium) chart helps to organize the given data and calculate the changes in concentration as the system reaches equilibrium.

For part b of the question, combining 2H+ and 2I− to make 2HI is incorrect in the context of dissociation or ionization reactions because these ions are formed as a result of the acid dissociation process and should be represented as individual ions in the chemical equation.