Question

Copper plating was accomplished using either graphite or copper as the electrodes. How would you expect the copper(II) ion concentration of the solution change (i.e. would [Cu2] increase, decrease, or remain the same?) during the plating process if the graphite anode were replaced with a copper one in the electrolysis of CuBr2? Explain your answer 5. Calculate the mass and thickness in mm of the chromium plate on an object if a current of 450.0 mamps were allowed to flow for 15.0 min. The plating solution contained chromium(III). Assume your object was a square solid 0.150 dm on an edge and of negligible thickness. The density of chromium is 7.15 g/cm. 6.

Answer 1

hen S s graphite is the ande which an inert ес and cathode γχ n is aa+ +2E →aus). T,erefore lcu2t). decreases as the elect10lys s trou ata proued 04 cu the onede, anode. Ten is ackve elechode) CS) Cathode 7xn is Cay Caat dato tue electroligta) There ore will remain Same untl all I Cuey med as anode is discolved Imol Cries! . 9%, gCr deposit 51.99 6gCr electolysis It deposits 3x 96, 48구 c ie 3F (or) = 51.996 lo00 ma = 405 c 51.996 g x 405c 3 × 96, 487 C Mass of C 405 C object is square wt eghgible tinceness. Hene totl area to be platad = &хаг.ta 느 edge) a2015odm x 1L almx 100 n KCleness . is Sauare = 1-5 cm 2x(15cm): of cr mekt 4.5 cm = -6.07 229-0010168 cmP volume

Thick ness Res af platryVolum e of metal Area of plata = 0.010168 cm 4S CM 00 225 cm ニ2-259 × 103 cm x 2. 26 xio3 cm 2.