1) ________use an externally generated electrical current to produce a chemical reaction that would not otherwise take place. a) Voltaic cells b) Electrolytic cells c) Salt bridges 2) The fundamental quantity of electrical charge on one mole of electrons used by chemists is a a) Faraday b) Pooraday c) Volt 3) Michael Faraday found that the mass of a substance produced by a redox reaction at an electrode is __________ the quantity of electrical charge that has passed through the electrochemical cell. a) less than b) the square root of c) proportional to 4) The charge on one mole of electrons is __________ Coulombs. a) 18600 b) 96500 c) 0.05916 5) Consider the reduction of Mn 7+ to Mn 2+. How many Faradays of electrical charge are needed? a) 2 b) 7 c) 5 6) A conclusion from Faraday's second law is that for a given quantity of electricity, the moles of substance produced __________ as the oxidation number increases. a) increase b) is equivalent c) decrease 7) The electrolysis of water produces a) Gaseous water’ b) H2 and O2 gases c) Electrically charged water 8) Electrolysis uses electrical current to a) Speed up a spontaneous reaction b) orce aForce a nonspontaneous reaction to occur c) Stop a spontaneous reaction from proceeding 9) Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milliampere current. The time required to liberate 0.01 mol of H2 gas at the cathode is:  a) 9.65 x 104s b) 28.95 x 104s c) 19.3 x 104s d) 38.6 x 104s 10) The electric charge for electrode deposition of one equivalent of the substance is: a) One ampere per second b) 96,500 Coulombs per second c) One ampere per hour d) Charge on 1 mole of electrons

FARADAY'S LAW

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