CHEM 107 Lecture Notes - Lecture 41: Galvanic Cell, Ionic Compound, Chemical Equation
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List of common strong acids and bases under useful handouts. Predict the products of each reaction, balance the equation, and determine which type of reaction it is (precipitation, redox, acid-base, or gas evolution) Hcl (aq) + k2co3 (aq) kcl(aq) + co2 (g) + h2o gas evolution. Li2co3 (aq) + cocl2 (aq) 2licl (aq) + coco3(s) Hclo4 (aq) + koh (aq) kclo4(aq) + h2o(l) K(s) + licl (aq) kcl(aq) + li(s) If the galvanic cell is constructed with a mn/mn2+ electrode and a cr/cr3+ electrode, determine which electrode will be the cathode and which electrode will be the anode. Write each half-cell reaction and the overall cell reaction. Write a net ionic equation for this reaction. H2so4 (aq) + 2naoh (aq) na2so4 (aq) + 2h2o (l) 2- (aq) + 2na+ (aq) + 2oh- (aq) 2na+ (aq) + so4. 2h+ (aq) + 2oh- (aq) 2h2o (l) H+ (aq) + oh- (aq) h2o (l)
