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18 Nov 2019
a. Formulate the expression for K, for the alternate reaction just cited. b. Find Ke as you did in Problem I; take due account of the fact that two moles SCN are used up per mole Fe(SCN), formed as you carry out the following calculations Step 1 Results are as in Problem 1 How many moles of Fe(SCN)2' are in the mixture at equilibrium? (This will be the same as in Problem 1.) Step 2 moles Fe(SCN) How many moles of Fe and SCN are used up in making the Fe(SCN),? mols Femoles SCN Step 3 How many moles of Fe and SCN remain in solution at equilibrium? Use the results of Steps and 2, noting that moles SCN at equilibrium riginal moles SCN--(2 à moles Fe(SCN)'). moles Fe":-- moles SCN- Step 4 what are the concentrations of Fe3·SCN-, and Fe(SCN)2 + at equilibrium? (Use Eq. 3 and the results of Step 3.) Step 5 Calculate K, based on the assumption that the alternate reaction occurs. (Use the answer to Part 2a.)
a. Formulate the expression for K, for the alternate reaction just cited. b. Find Ke as you did in Problem I; take due account of the fact that two moles SCN are used up per mole Fe(SCN), formed as you carry out the following calculations Step 1 Results are as in Problem 1 How many moles of Fe(SCN)2' are in the mixture at equilibrium? (This will be the same as in Problem 1.) Step 2 moles Fe(SCN) How many moles of Fe and SCN are used up in making the Fe(SCN),? mols Femoles SCN Step 3 How many moles of Fe and SCN remain in solution at equilibrium? Use the results of Steps and 2, noting that moles SCN at equilibrium riginal moles SCN--(2 à moles Fe(SCN)'). moles Fe":-- moles SCN- Step 4 what are the concentrations of Fe3·SCN-, and Fe(SCN)2 + at equilibrium? (Use Eq. 3 and the results of Step 3.) Step 5 Calculate K, based on the assumption that the alternate reaction occurs. (Use the answer to Part 2a.)
Reid WolffLv2
20 Apr 2019