1. In the electrolysis of molten sodium chloride,
sodium metal is produced at the anode & chlorine gas at the cathode
sodium ions are produced at the cathode & chloride at the anode
sodium ions are produced at the anode & chloride at the cathode
sodium metal is produced at the cathode & chlorine gas at the anode ***
2.An electrolytic cell can be used to
generate electricity
store electricity
make a battery
electroplate an object that conducts electricity***
3. A non-rechargeable battery won't recharge. This must be because...
as it's used, the chemicals inside it disappear***
it can't conduct electricity
a non-soluble product forms while it is used
non-rechargeable batteries don't have a salt bridge
4.To determine the useful energy available in a voltaic cell, use this formula:
∆G=-nFE
E=E°-(RT/nF)lnQ***
E=E°-0.0592/nlogQ
W=J/s
I agree with your answers to 1 and 2. I think your choice for 3 is the best one available but I don't like the wording about chemicals disappearing. They change into other forms but they don't really disappear. I don't agree with your choice for 4. Your choice (that's b) calculates volts. Choice c is the same thing because [RT/nF*ln] Q converts to [0.0592/n*log] Q. Delta G is the useful work of a system.
1. The correct answer is "sodium metal is produced at the cathode & chlorine gas at the anode." This can be determined by the process of electrolysis, where an electric current is passed through a molten sodium chloride solution. The positive sodium ions (Na+) are attracted to the negative cathode, where they gain electrons, lose their charge, and form sodium metal (Na). On the other hand, the negative chloride ions (Cl-) move towards the positive anode, where they lose electrons, gain a charge, and form chlorine gas (Cl2).
2. The correct answer is "electroplate an object that conducts electricity." An electrolytic cell is a setup in which an electric current is used to drive a non-spontaneous chemical reaction. This process can be used to electroplate an object by passing an electric current through a solution containing metal ions. The metal ions are attracted to the object being electroplated (the cathode), where they deposit onto the surface, creating a thin layer of metal.
3. The correct answer is "as it's used, the chemicals inside it disappear." Non-rechargeable batteries, also known as primary batteries, are designed to be used until the chemicals inside them are no longer capable of producing an electric current. As the battery is used, the chemicals undergo irreversible chemical reactions, depleting the reactants (such as the chemicals in the electrodes) and rendering the battery unable to be recharged.
4. The correct answer is "∆G=-nFE." This formula represents the Gibbs free energy change (∆G) of a voltaic (or galvanic) cell, which is a type of electrochemical cell that converts chemical energy into electrical energy. The formula incorporates the number of moles of electrons transferred (n), the Faraday constant (F), and the cell potential (E), which can be determined using other equations depending on the given conditions. The other options presented are not applicable formulas for determining the useful energy available in a voltaic cell. The unit "W=J/s" stands for power, not energy.