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In acidic medium, dichromate oxidizes ferrous ions to ferric ion. If molecular weight of potassium dichromate is 294, its equivalent weight would be?
Correct answer is '49'. Can you explain this answer?
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In acidic medium, dichromate oxidizes ferrous ions to ferric ion. If m...
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In acidic medium, dichromate oxidizes ferrous ions to ferric ion. If m...
Explanation:
1. Understanding the concept of equivalent weight:
Equivalent weight is a concept used in stoichiometry to determine the amount of a substance required to react with or be replaced by one mole of another substance. It is calculated by dividing the molar mass of a substance by its valence or the number of electrons involved in the reaction.
2. Determining the valence of potassium dichromate:
Potassium dichromate (K2Cr2O7) contains two potassium ions (K+) and one dichromate ion (Cr2O7^2-). The dichromate ion has a -2 charge, so each chromium atom has a +6 charge. This means that the valence or the number of electrons involved in the reaction is 6.
3. Calculating the molecular weight of potassium dichromate:
To find the molecular weight of potassium dichromate, we add the atomic masses of all the elements present in the compound:
2(K) + 2(Cr) + 7(O) = 39.1(2) + 52(2) + 16(7) = 294 g/mol
4. Calculating the equivalent weight:
To calculate the equivalent weight, we divide the molecular weight by the valence:
Equivalent weight = Molecular weight / Valence
Equivalent weight = 294 g/mol / 6 = 49 g/mol
Therefore, the equivalent weight of potassium dichromate is 49 g/mol. This means that 49 grams of potassium dichromate are required to oxidize one mole of ferrous ions to ferric ions in an acidic medium.
1. Understanding the concept of equivalent weight:
Equivalent weight is a concept used in stoichiometry to determine the amount of a substance required to react with or be replaced by one mole of another substance. It is calculated by dividing the molar mass of a substance by its valence or the number of electrons involved in the reaction.
2. Determining the valence of potassium dichromate:
Potassium dichromate (K2Cr2O7) contains two potassium ions (K+) and one dichromate ion (Cr2O7^2-). The dichromate ion has a -2 charge, so each chromium atom has a +6 charge. This means that the valence or the number of electrons involved in the reaction is 6.
3. Calculating the molecular weight of potassium dichromate:
To find the molecular weight of potassium dichromate, we add the atomic masses of all the elements present in the compound:
2(K) + 2(Cr) + 7(O) = 39.1(2) + 52(2) + 16(7) = 294 g/mol
4. Calculating the equivalent weight:
To calculate the equivalent weight, we divide the molecular weight by the valence:
Equivalent weight = Molecular weight / Valence
Equivalent weight = 294 g/mol / 6 = 49 g/mol
Therefore, the equivalent weight of potassium dichromate is 49 g/mol. This means that 49 grams of potassium dichromate are required to oxidize one mole of ferrous ions to ferric ions in an acidic medium.
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In acidic medium, dichromate oxidizes ferrous ions to ferric ion. If molecular weight of potassium dichromate is 294, its equivalent weight would be?Correct answer is '49'. Can you explain this answer?
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