Chemistry, 28.06.2019 03:40 cristabean87
Calculate the cell potential, e, for the following reactions at 26.29 °c using the ion concentrations provided. then, determine if the cells are spontaneous or nonspontaneous as written. standard reduction potentials (e°red) may be found here.'1) pt(s)+fe2+(aq)\rightleftharpoonspt2 + (aq)+fe(s)[fe2+]=0.0066m [pt2+]=0.057me= ? v2) cu(s)+2ag+(aq)\rightleftharpoonscu2 +(aq)+2ag(s)[cu2+]=0.013m [ag+]=0.013me= ? v3) co2+(aq)+ti3+(aq)\rightleftharpoons co3+(aq)+ti2+(aq)[co2+]=0.050m [co3+]=0.030m[ti3+]=0.0055m [ti2+]=0.0110me=? vcalculate the cell potential for the following reaction as written at 25.00 °c, given that [mg2 ] = 0.796 m and [sn2 ] = 0.0170 m. standard reduction potentials can be found here. mg(s)+sn2+(aq)\rightleftharpoonsmg2 +(aq)+sn(s)e=? v
Answers: 2
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One of the few xenon compounds that form is cesium xenon heptafluoride (csxef7). how many moles of csxef7 can be produced from the reaction of 13.0 mol cesium fluoride with 12.5 mol xenon hexafluoride? csf(s) + xef6(s) csxef7(s)
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17) large amounts of very important metal titanium are made by reacting magnesium metal with titanium tetrachloride. titanium metal and magnesium chloride are produced. a) write the balanced equation for this reaction. b) how many kilograms of magnesium are required to produce 1.00 kilograms of titanium? ( show work, .)
Answers: 1
Calculate the cell potential, e, for the following reactions at 26.29 °c using the ion concentration...
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