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The equilibrium constant for the following reaction at `25^(@)C " is " 2.9 xx 10^(9)`. Calculate standard voltage of the cell. `C1_(2(g)) + 2Br_((aq))^(-) hArr Br_(2(1)) + 2C1_((aq))^(-)` |
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Answer» Correct Answer - Standard voltage of the cell `=E_("cell ")^(0) = 0.28 V` Given : Cell reaction `:C1_(2(g)) + 2Br_((aq))^(-) hArr Br_(2(1)) + 2C1_((aq))^(-)` Equilibrium constant = k = 2.9 `xx10^(-9) atm ^(-1)` Standard voltage of the cell = `E_("cell ")^(0) = ? ` The formulation of the cell : `Pt|Br_(2(1)) | (1M)" ||"C1_((aq))^(-) (1M)|C1_(2) (g,P_(C1_(2))) | Pt` `((LHE 2Br_((aq))^(-) to Br_(2(1)) + 2e^(-))/(RHE . C1_(2(g)) + 2e^(-) to 2C1_((aq))^(-)))/(2Br_((aq))^(-) + C1_(2(g)) to Br_(2(1))+ 2C1_((aq))^(-))" "underset"(Overall cell reaction )"underset"(Reduction at cathode )"("(Oxidation at anode)")` `:. n=2` `E_("cell ")^(0) = (0.0592)/(n) log_(10) K` `= (0.0592)/(2) log_(10) 2.9 xx 10^(9)` `=0. 0296 xx (9.4624)` `=0.28 V` |
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