Exercise 16.45 - Enhanced - with Feedback MISSED THIS? Read Section 16.6 (Pages 696 - 699); Watch IWE 16.5 Consider the

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Exercise 16 45 Enhanced With Feedback Missed This Read Section 16 6 Pages 696 699 Watch Iwe 16 5 Consider The 1 (83.96 KiB) Viewed 10 times

Exercise 16.45 - Enhanced - with Feedback MISSED THIS? Read Section 16.6 (Pages 696 - 699); Watch IWE 16.5 Consider the reaction H₂(g) + I₂(g) = 2HI(g) A reaction mixture in a 3.610-L flask at a certain temperature initially contains 0.7640 g H₂ and 97.10 g I₂. At equilibrium, the flask contains 90.40 g HI. Part A Calculate the equilibrium constant (K) for the reaction at this temperature. Express your answer to two significant figures. IVE ΑΣΦ S Kc = 578 Submit Previous Answers Request Answer X Incorrect; Try Again Prepare an ICE table that shows the known concentrations you need to calculate first: [12] ? Initial Change Equilibrium Provide Feedback 11 of 33 Review Constants | Periodic Table 0.000 > You will need to convert the three masses given to concentration (in mol/L) given the molar mass of each species (in g/mol) and the volume of the reaction mixture (3.610 L). The concentration calculated for HI is equivalent to its change in concentration, since no product was in the flask initially. Use this value and the stoichiometric relationships from the balanced chemical equation to determine the change in concentration of each reactant. Then find the equilibrium concentration of each reactant. Finally, substitute the equilibrium concentrations into the K, expression for the given reaction. Next >