QUESTION #13-#19 ARE BASED OF THE FOLLOWING EXPERIMENTAL RESULTS: A student did

Question

QUESTION #13-#19 ARE BASED OF THE FOLLOWING EXPERIMENTAL RESULTS: A student did an experiment to find the equilibrium constant K of the following reaction: Fe+(aq) +SCN (aq)FeSCN+(aq) thiocyanoiron III) iron(III) thiocyanate He prepared the following solutions using 0.0020 M Fe(NO3) AND 0.0020 KSCN and measured their absorbance: Number m) )m He also prepared a standard solution of FeSCN+ by pipetting 18 mL of 0.200 M Fe(NO3)3 into a 20 X 150 mm test tube labeled "5". Pipet 2 mL of 0.0020 M KSCN into the same test tube and measured its absorbance. He collected the following data for trials 1 and 2 TUBE 1 T TUBE 2 0.153 of standard (Test tube 5) 13. Write the Equilibrium constant expression, Kc, for this reaction. (1pt) 14. Calculate the initial concentration of Fe, based on the dilution that results from adding KSCN solution and water to the original 0.0020 M Fe(NO solution. Calculate [Fe3+]i using the equation: [Fe]i- X (0.0020 M) (2pts) This should be the same for all two test tubes. Dashboard Calendar To Do Notifications Inbox

Explanation / Answer

13. At equilibrium and at a given temperature, the relationship between the amounts of products and reactants present, in a reversible chemical reaction, is expressed as its equilibrium constant Kc.

Thus, Kc = [FeSCN2+] / {[Fe3+][SCN-]}

14. [Fe3+]i = 0.002 mol/L * (5mL +3 mL+ 2mL)

=  0.002 mol/L * 10mL

=  0.002 mol/L * 0.01L

= 0.00002 mol

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