9th Class Chemistry Chapter 7 Electrochemistry Short Questions Answer
Chapter 7 of the 9th grade chemistry textbook explores the interesting field of electrochemistry, revealing the complex relationship between chemical processes and electrical currents. So we are providing here the 9th Class Chemistry Chapter 7 Electrochemistry Short Questions Answer for students of 7th class. As the scientific link between the fields of chemistry and electricity, electrochemistry studies the conversion of chemical energy into electrical energy and the other way around. The concepts that underpin electrolysis, redox processes, and the creation of electrical potential are all explained in this chapter. Students study the fundamental roles of ions, electrons, and the electrochemical series as they set off on this fascinating adventure, providing the groundwork for a greater understanding of the fascinating world at the molecular level.
9th Class Chemistry Chapter 7 Electrochemistry Short Questions Answer
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Here we are providing complete chapter wise Chemistry questions and Answers for the 9th class students. All the visitors can prepare for their 9th class examination by attempting below given question answers.
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- Lahore Board 9th class Chapter 7 Electrochemistry short questions Answer
- Rawalpindi Board 9th class Chapter 7 Electrochemistry short questions Answer
- Gujranwala Board 9th class Chapter 7 Electrochemistry short questions Answer
- Multan Board 9th class Chapter 7 Electrochemistry short questions Answer
- Sargodha Board 9th class Chapter 7 Electrochemistry short questions Answer
- Faisalabad Board 9th class Chapter 7 Electrochemistry short questions Answer
- Sahiwal Board 9th class Chapter 7 Electrochemistry short questions Answer
- DG Khan Board 9th class Chapter 7 Electrochemistry short questions Answer
- Bahawalpur Board 9th class Chapter 7 Electrochemistry short questions Answer
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Oxidation is the loss of electron by an atom or an ion e.g,
Reduction is defined as:
“The addition of hydrogen or removal of oxygen during a chemical reaction.”
Valency:
The apparent charge on an atom, ion or molecule which is called valency.
Valency is written as the sign followed by the number as valency = OII²
Oxidation:
The apparent charge assigned to an atom of an element in a molecule or an ion.
No sign
Oxidizing agents:
These are the substance that reduce itself and oxidize other.
They gain the electrons.
Non-metals are good oxidizing agent
They are more electronegative in nature.
Reducing Agent:
These are the substance that oxidize itself and reduce other.
They loss the electrons.
Metals are good reducing agents.
They are mostly electropositive.
Strong electrolyte:
Definition: The electrolyte which ionize completely in solution and produce more ions, are called strong electrolyte.
Example strong electrolytes are aqueous of NaCI, NaOH, and H₂SO₄
Weak electrolyte:
Definition: The electrolyte which ionize to a small extent when dissolve in water and could not produce more ions are called weak electrolytes.
Example: Weak electrolyte are the aqueous solution of acetic acid or Ca(OH₂)
It involves the dipping of the clean sheet of ion in a both of molten tin and then passing it through pair of rollers.
The steel is usually plated first with nickel or copper then by chromium because it does not adhere well on the steel surface. Moreover, it allows moisture to pass through it and metal is stripped off.
According to the definition of oxidation:
“The loss of electron is called oxidation” in the above reaction.
“Al° with zero oxidation state changes to AI⁺³ mean it losses 3 electron, so, the oxidation reaction takes place”.
Example:
In the above reaction, loss of electron takes place, chloride ion, (anion) convert into chlorine molecule by losing electrons. So oxidation takes place
In case of galvanic ell, anode release the electrons, that gathered at anode and create negative charge while in case of electrolytic cell, the anode attached to the positive terminal of the battery, that is why, it carry positive charge.
In Daniel cell, the electrons takes flow from Zn electrode (anode) towards the cathode made up of copper.
In galvanic cell, oxidation takes place at anode while reduction takes place at cathode. And oxidation always takes place at anode while reduction always takes place at cathode.
In galvanic cell, reduction takes place at the cathode as:
Brine (aqueous solution of NaCI called brine) is used as electrolyte in Nelson’s cell.
Hydrogen gas (H₂) and chlorine gas (Cl₂) are the by-product of Nelson’s cell as
Galvanizing is done to protect the iron against corrosion.
Iron grill is painted frequently because due to presence of oxygen water in air, it become corrode, so to prevent it from rusting, it is painted.
Oxygen plays important rule in rusting. Electrons reduce the oxygen molecules in the presence of H⁺ ions.
Chromium sulphate with few drops of H₂SO₄ acts electrolyte.
In electroplating of silver Ag⁺ ion come form anode while they deposit at cathode.
The electrolyte is the solution of chromium sulphate Cr₂(SO₄)a few drops of H₂SO₄ are added in the electrolyte to prevent its hydrolyses, while the object to be electroplated acts as cathode and anode is made of antimonies lead.
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