Simple chemical cells involve two electrodes. Which of the following statements is correct?Both electrodes must be carbonThe electrodes must be two different metalsOne electrode must be carbonThe electrodes must be the same metal2To make a chemical cell, two metal electrodes are dipped in a salt or dilute acid solution and joined by a wire. What causes the electrical current?The flow of electrons from the more reactive metal to the less reactive metalThe formation of metal ions in the salt solutionThe flow of electrons from the less reactive metal to the more reactive metalThe loss of heat to the surroundings3A zinc/carbon chemical cell (or battery) contains a paste of ammonium chloride. What is the function of this paste?To hold the electrodes in placeTo hold the wire in placeTo act as an electrolyteTo act as an electrode4What is the balanced equation of the overall reaction that takes place in a fuel cell?H2 + O2 → H2O2H2O → 2H2 + O22H2 + O → 2H2O2H2 + O2 → 2H2O5Which of the following is a disadvantage of using hydrogen as a fuel?Hydrogen gas is highly flammableFuel cells can be a range of sizesThe only waste product is waterFuel cells do not require recharging6Which of the following statements about hydrogen-oxygen fuel cells is not true?The only waste product is waterAn acidic electrolyte is requiredHydrogen must be supplied constantlyElectrical energy is produced from the oxidation of hydrogen
Question
Simple chemical cells involve two electrodes. Which of the following statements is correct?Both electrodes must be carbonThe electrodes must be two different metalsOne electrode must be carbonThe electrodes must be the same metal2To make a chemical cell, two metal electrodes are dipped in a salt or dilute acid solution and joined by a wire. What causes the electrical current?The flow of electrons from the more reactive metal to the less reactive metalThe formation of metal ions in the salt solutionThe flow of electrons from the less reactive metal to the more reactive metalThe loss of heat to the surroundings3A zinc/carbon chemical cell (or battery) contains a paste of ammonium chloride. What is the function of this paste?To hold the electrodes in placeTo hold the wire in placeTo act as an electrolyteTo act as an electrode4What is the balanced equation of the overall reaction that takes place in a fuel cell?H2 + O2 → H2O2H2O → 2H2 + O22H2 + O → 2H2O2H2 + O2 → 2H2O5Which of the following is a disadvantage of using hydrogen as a fuel?Hydrogen gas is highly flammableFuel cells can be a range of sizesThe only waste product is waterFuel cells do not require recharging6Which of the following statements about hydrogen-oxygen fuel cells is not true?The only waste product is waterAn acidic electrolyte is requiredHydrogen must be supplied constantlyElectrical energy is produced from the oxidation of hydrogen
Solution
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The correct statement is: The electrodes must be two different metals. In a simple chemical cell, the two electrodes are usually made of different metals which react differently with the electrolyte, causing a flow of electrons and thus, creating an electric current.
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The electrical current in a chemical cell is caused by: The flow of electrons from the more reactive metal to the less reactive metal. This is because the more reactive metal tends to lose electrons (oxidation) which then flow to the less reactive metal (reduction).
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The function of the ammonium chloride paste in a zinc/carbon chemical cell is: To act as an electrolyte. An electrolyte is a substance that produces an electrically conducting solution when dissolved in a polar solvent.
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The balanced equation of the overall reaction that takes place in a fuel cell is: 2H2 + O2 → 2H2O. This represents the reaction of hydrogen with oxygen to produce water, which is the basic principle of a hydrogen fuel cell.
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A disadvantage of using hydrogen as a fuel is: Hydrogen gas is highly flammable. This makes it potentially dangerous to use and store.
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The statement about hydrogen-oxygen fuel cells that is not true is: Electrical energy is produced from the oxidation of hydrogen. In fact, electrical energy is produced from the combination of oxidation of hydrogen at the anode and reduction of oxygen at the cathode.
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