# An electrochemical cell was found to have a cell

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An electrochemical cell was found to have a cell potential ( E cell ) of 1.75 V and the number of electrons transferred (n) was 2. What is the change in free energy ( G) of the cell in kJ? G = - nFE cell G =___-338 kJ ____ 7. Calculate the molar solubility of PbCl 2 (K sp = 1.7x10 -5 ) in pure water K sp = [Pb 2+ ][Cl 1- ] 2 x (PbCl 2 ) = ³√(K sp /4) x (PbCl 2 ) = ___0.016 M ____ Calculate the molar solubility of TlCl (K sp = 1.9x10 -4 ) in pure water K sp = [Tl 1+ ][Cl 1- ] x (TlCl) = √(K sp ) x (TlCl) = ____0.014 M ___ Circle the less soluble salt: PbCl 2 / TlCl At what [Cl 1- ] will PbCl 2 begin to precipitate out of a 0.15 M solution of Pb 2+ ? [Cl 1- ] = √(K sp / [Pb 2+ ]) [Cl 1- ] = ___0.0106 M __

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CH201-001 SSII 2009 Name:____________________________________ Exam 3 Last First 8. Using the data in the chart below, write out the rate law expression for the following reaction: H 2 SeO 3 (aq) + 6I 1- (aq) + 4H 1+ (aq) Se(s) + 2I 3 1- (aq) + 3H 2 O(l) Rate = k[H 2 SeO 3 ] x [I 1- ] y [H 1+ ] z x = 1, y = 1, z = 2 Rate = __ Rate = k [H 2 SeO 3 ][I 1- ][H 1+ ] 2 ____ Given that ( [I 3 1- ]/ t) = 1.52x10 -3 , what is the rate of disappearance of I 1- , H 2 SeO 3 and the rate of reaction? -( [I 1- ]/ t) = ____4.56x10 -3 Ms -1 _____ -( [H 2 SeO 3 ]/ t) = ____7.60x10 -4 Ms -1 _____ Rate = ____7.60x10 -4 Ms -1 _____ Calculate a numeric value for k (be sure to include proper units for k) Plug in numbers from the data table into the “Rate” [H 2 SeO 3 ], M [I 1- ], M [H 1+ ], M Rate of I 3 1- formation, Ms -1 0.140 0.230 0.100 1.52 × 10 -3 0.280 0.230 0.100 3.04 × 10 -3 0.140 0.460 0.100 3.04 × 10 -3 0.140 0.230 0.200 6.08x10 -3
CH201-001 SSII 2009 Name:____________________________________ Exam 3 Last First k = ____2.36 M -3 s -1 _______ 9. The kinetics of the reaction A B was studied by monitoring [A] as a function of time. The following graphs were constructed from the data.

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