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Principle of Electroplating: The principle of electroplating is based on the reduction of metal ions at the cathode (the object to be plated) in an electrolytic cell. When a direct current is passed through an electrolyte solution containing metal ions, the metal ions are reduced onto the surface of the object, forming a thin, adherent … Read more
Electroplating is the process of depositing a thin layer of metal onto the surface of an object using an electrical current. The metal is deposited from a solution containing its ions. Electroplating is commonly used to improve the appearance, prevent corrosion, reduce friction, or increase the hardness of the object being plated. Procedure for Electroplating: … Read more
Galvanizing and tin plating are two methods used to protect iron or steel from corrosion, but galvanizing is generally considered to be more effective than tin plating for several reasons: Galvanizing: Galvanizing involves coating iron or steel with a layer of zinc. This process is typically done through hot-dip galvanizing, where the metal is dipped … Read more
The rusting of iron is a type of oxidation-reduction (redox) reaction that occurs when iron reacts with oxygen and water in the environment. This process leads to the formation of iron oxides, commonly known as rust. Rusting is a complex electrochemical process that can be broken down into two main half-reactions: oxidation at the anode … Read more
The commercial preparation of sodium hydroxide (NaOH) is primarily done through the chloralkali process. This process involves the electrolysis of sodium chloride (NaCl) solution (brine) to produce sodium hydroxide, chlorine gas, and hydrogen gas. Chemistry of the Process: Electrolysis of Brine: Brine is subjected to electrolysis in an electrolytic cell with a diaphragm or membrane … Read more
A cell that produces electricity is known as a galvanic cell or voltaic cell. It converts chemical energy into electrical energy through a spontaneous redox reaction. A common example of a galvanic cell is the Daniel cell, which uses zinc and copper electrodes. Construction: Two half-cells: A galvanic cell consists of two half-cells, each containing … Read more
The electrolysis of water involves the decomposition of water (H₂O) into hydrogen gas (H₂) and oxygen gas (O₂) using electrical energy. This is a non-spontaneous reaction, requiring an electrolytic cell. Reaction: 2H2O(l)→electrolysis→2H2(g)+O2(g) Process: Electrolytic Cell Setup: The cell consists of two electrodes—an anode (positive electrode) and a cathode (negative electrode)—placed in water with an electrolyte … Read more
A non-spontaneous reaction is one that does not occur naturally under standard conditions, meaning it requires an input of external energy to proceed. This is where electrolysis comes into play, allowing non-spontaneous reactions to occur by supplying electrical energy. Electrolysis is a process in which electrical energy is used to drive a chemical reaction that … Read more
(a) Na₂SO₄ (S) Sodium (Na) has an oxidation state of +1 (since it’s a Group 1 element). Oxygen (O) has an oxidation state of -2. Let the oxidation state of sulfur (S) be xxx. The sum of the oxidation states in a neutral compound is zero: 2(+1)+x+4(−2)=0 2+x−8=0 x=+6 So, sulfur has an oxidation state … Read more
Calcium metal reacts with dilute sulfuric acid (H₂SO₄) to produce calcium sulfate (CaSO₄), hydrogen gas (H₂), and heat. The reaction can be written as: Ca(s)+H2SO4(aq)→CaSO4(aq)+H2(g). The reaction is vigorous, and hydrogen gas is released, which can be detected by its characteristic “pop” sound when exposed to a flame. Related Questions: Choose Arrhenius acids from the … Read more