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50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas to sulphur. Volume of 0.03 M KMnO4 required to oxidise the same amount of H2S gas to sulphur in acidic medium is 10 x x. Here, the value of x is
Correct answer is '8'. Can you explain this answer?
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50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas ...
Milliequivalents of K2Cr2O7 reacted with H2S (N1V1) = miliiequivalents of KMnO4 reacted with H2S(N2V2), i.e. milliequivalent of KMnO4 = milliequivalent of H2S Therefore, 50 x 0.04 x 6 = V2 x 0.03 x 5
or V2 = 80 mL
or V2 = 80 mL
Most Upvoted Answer
50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas ...
To find the value of x in the given question, let's break down the problem into smaller steps:
Step 1: Write the balanced chemical equation for the reaction between H2S and K2Cr2O7 in acidic medium.
K2Cr2O7 + 4H2SO4 + 3H2S -> Cr2(SO4)3 + K2SO4 + 7H2O + 3S
Step 2: Calculate the number of moles of K2Cr2O7 used.
Given volume = 50 cc = 50/1000 L = 0.05 L
Molarity of K2Cr2O7 = 0.04 M
Number of moles of K2Cr2O7 = Molarity * Volume = 0.04 * 0.05 = 0.002 moles
Step 3: Determine the ratio between K2Cr2O7 and KMnO4.
From the balanced equation, we can see that 1 mole of K2Cr2O7 reacts with 1 mole of KMnO4 to oxidize H2S to sulfur.
Step 4: Calculate the number of moles of KMnO4 required.
Number of moles of KMnO4 = Number of moles of K2Cr2O7 = 0.002 moles
Step 5: Find the volume of 0.03 M KMnO4 required.
Molarity of KMnO4 = 0.03 M
Volume of KMnO4 required = Number of moles of KMnO4 / Molarity = 0.002 / 0.03 = 0.0667 L
Convert volume to cc: 0.0667 L * 1000 = 66.7 cc
Step 6: Calculate the value of x.
x = Volume of KMnO4 required / Volume of K2Cr2O7 used = 66.7 / 50 = 1.334
The value of x is not 8 as mentioned in the correct answer.
It seems there might be an error in the question or answer given. Please verify the information provided or provide additional context to resolve the discrepancy.
Step 1: Write the balanced chemical equation for the reaction between H2S and K2Cr2O7 in acidic medium.
K2Cr2O7 + 4H2SO4 + 3H2S -> Cr2(SO4)3 + K2SO4 + 7H2O + 3S
Step 2: Calculate the number of moles of K2Cr2O7 used.
Given volume = 50 cc = 50/1000 L = 0.05 L
Molarity of K2Cr2O7 = 0.04 M
Number of moles of K2Cr2O7 = Molarity * Volume = 0.04 * 0.05 = 0.002 moles
Step 3: Determine the ratio between K2Cr2O7 and KMnO4.
From the balanced equation, we can see that 1 mole of K2Cr2O7 reacts with 1 mole of KMnO4 to oxidize H2S to sulfur.
Step 4: Calculate the number of moles of KMnO4 required.
Number of moles of KMnO4 = Number of moles of K2Cr2O7 = 0.002 moles
Step 5: Find the volume of 0.03 M KMnO4 required.
Molarity of KMnO4 = 0.03 M
Volume of KMnO4 required = Number of moles of KMnO4 / Molarity = 0.002 / 0.03 = 0.0667 L
Convert volume to cc: 0.0667 L * 1000 = 66.7 cc
Step 6: Calculate the value of x.
x = Volume of KMnO4 required / Volume of K2Cr2O7 used = 66.7 / 50 = 1.334
The value of x is not 8 as mentioned in the correct answer.
It seems there might be an error in the question or answer given. Please verify the information provided or provide additional context to resolve the discrepancy.
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50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas to sulphur. Volume of 0.03 M KMnO4 required to oxidise the same amount of H2S gas to sulphur in acidic medium is 10 x x. Here, the value of x isCorrect answer is '8'. Can you explain this answer?
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50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas to sulphur. Volume of 0.03 M KMnO4 required to oxidise the same amount of H2S gas to sulphur in acidic medium is 10 x x. Here, the value of x isCorrect answer is '8'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about 50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas to sulphur. Volume of 0.03 M KMnO4 required to oxidise the same amount of H2S gas to sulphur in acidic medium is 10 x x. Here, the value of x isCorrect answer is '8'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas to sulphur. Volume of 0.03 M KMnO4 required to oxidise the same amount of H2S gas to sulphur in acidic medium is 10 x x. Here, the value of x isCorrect answer is '8'. Can you explain this answer?.
50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas to sulphur. Volume of 0.03 M KMnO4 required to oxidise the same amount of H2S gas to sulphur in acidic medium is 10 x x. Here, the value of x isCorrect answer is '8'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about 50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas to sulphur. Volume of 0.03 M KMnO4 required to oxidise the same amount of H2S gas to sulphur in acidic medium is 10 x x. Here, the value of x isCorrect answer is '8'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas to sulphur. Volume of 0.03 M KMnO4 required to oxidise the same amount of H2S gas to sulphur in acidic medium is 10 x x. Here, the value of x isCorrect answer is '8'. Can you explain this answer?.
Solutions for 50 cc of 0.04 M K2Cr2O7 in acidic medium oxidises a sample of H2S gas to sulphur. Volume of 0.03 M KMnO4 required to oxidise the same amount of H2S gas to sulphur in acidic medium is 10 x x. Here, the value of x isCorrect answer is '8'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 12.
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