. Electrical news and engineering . If we know the electro-chemical equivalent of any ele-ment, and we also know the chemical equivalent of the othermetals, the electro-chemical equivalent of these metals can readilybe calculated. It has been determined experimentally i coulomb, passingthrough water, will liberate .000010352 grams of hydrogen, andas the chemical equivalent of copper is , therefore the electro-chemical equivalent will be = chem. equiv. x .000010352 = .00032-6088, and so on, for the rest of the metals. If we suppose thefour cells in Fig. i to be copper, zinc, nickel an
. Electrical news and engineering . If we know the electro-chemical equivalent of any ele-ment, and we also know the chemical equivalent of the othermetals, the electro-chemical equivalent of these metals can readilybe calculated. It has been determined experimentally i coulomb, passingthrough water, will liberate .000010352 grams of hydrogen, andas the chemical equivalent of copper is , therefore the electro-chemical equivalent will be = chem. equiv. x .000010352 = .00032-6088, and so on, for the rest of the metals. If we suppose thefour cells in Fig. i to be copper, zinc, nickel and silver, wehave a deposit grams in the copper, 121 in the zinc, i 10 inthe nickel, and grams in the silver voltameter, we can deter-mine the ampere-hours. Let C — current, y = electro-chemical equivalent, t = time in second and M = mass decomposed, then C = -, or taking the copper voltameter, we have C = r-^-^—; = °° amperes ^^ .0003261 X 1 hour flowing for one hour or equivalent thereto. If the current in each. FI&URE Z of these four cells calculates out to be the same, then we mustcome to the correct conclusion that 100 amperes must have passedfor one hour, or equivalent thereto. If only one of these volta-meters had been in the circuit and the resistance remaining thesame, we would have had exactly the same results. In the aboveexample of a derived circuit composed of i and 2 ohms, we placethe copper voltameter in the 2 ohms branch, and we find as above, grams deposit, which represents too ampere hours; then asthis only represents one-third of the total current passed throughthe circuit, therefore 300 ampere hours would be the correct read-ing on this particular meter. With this pieliminary and elementary explanation we are nowin a position to more clearly understand the chemical meter and July, 1896 CANflDlflN EbECTI^lCMb fJEWS also to follow up some of those as made by Edison. It will, how-ever, be entirely out of the question to treat on all the me
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