UPSC Exam > UPSC Questions > When 11.2 g of iron combines with sulphur, 17...
Start Learning for Free
When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is?
Most Upvoted Answer
When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is ...
Calculating the number of equivalents in iron
Iron and sulfur react to form iron sulfide according to the equation:
Fe + S → FeS
Given that 11.2 g of iron combines with sulfur to form 17.6 g of iron sulfide, we can calculate the number of equivalents present in 11.2 g of iron.
Step 1: Calculate the molar mass of Fe and FeS
- The molar mass of Fe (iron) is 55.85 g/mol.
- The molar mass of FeS (iron sulfide) is 87.91 g/mol (55.85 g/mol + 32.06 g/mol).
Step 2: Calculate the number of moles of Fe and FeS
- Number of moles of Fe = 11.2 g / 55.85 g/mol = 0.2 moles
- Number of moles of FeS = 17.6 g / 87.91 g/mol = 0.2 moles
Step 3: Determine the limiting reactant
- In this case, both Fe and FeS have the same number of moles, so Fe is the limiting reactant.
Step 4: Calculate the number of equivalents of Fe
- Since Fe is the limiting reactant, the number of equivalents of Fe is equal to the number of moles of Fe.
- Therefore, the number of equivalents present in 11.2 g of iron is 0.2 equivalents.
By following these steps, we can determine the number of equivalents present in a given mass of iron when it reacts with sulfur to form iron sulfide.
Iron and sulfur react to form iron sulfide according to the equation:
Fe + S → FeS
Given that 11.2 g of iron combines with sulfur to form 17.6 g of iron sulfide, we can calculate the number of equivalents present in 11.2 g of iron.
Step 1: Calculate the molar mass of Fe and FeS
- The molar mass of Fe (iron) is 55.85 g/mol.
- The molar mass of FeS (iron sulfide) is 87.91 g/mol (55.85 g/mol + 32.06 g/mol).
Step 2: Calculate the number of moles of Fe and FeS
- Number of moles of Fe = 11.2 g / 55.85 g/mol = 0.2 moles
- Number of moles of FeS = 17.6 g / 87.91 g/mol = 0.2 moles
Step 3: Determine the limiting reactant
- In this case, both Fe and FeS have the same number of moles, so Fe is the limiting reactant.
Step 4: Calculate the number of equivalents of Fe
- Since Fe is the limiting reactant, the number of equivalents of Fe is equal to the number of moles of Fe.
- Therefore, the number of equivalents present in 11.2 g of iron is 0.2 equivalents.
By following these steps, we can determine the number of equivalents present in a given mass of iron when it reacts with sulfur to form iron sulfide.
Attention UPSC Students!
To make sure you are not studying endlessly, EduRev has designed UPSC study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in UPSC.
|
Explore Courses for UPSC exam
|
|
Similar UPSC Doubts
Top Courses for UPSCView all
When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is?
Question Description
When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is? for UPSC 2024 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is? covers all topics & solutions for UPSC 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is?.
When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is? for UPSC 2024 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is? covers all topics & solutions for UPSC 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is?.
Solutions for When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is? in English & in Hindi are available as part of our courses for UPSC.
Download more important topics, notes, lectures and mock test series for UPSC Exam by signing up for free.
Here you can find the meaning of When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is? defined & explained in the simplest way possible. Besides giving the explanation of
When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is?, a detailed solution for When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is? has been provided alongside types of When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is? theory, EduRev gives you an
ample number of questions to practice When 11.2 g of iron combines with sulphur, 17.6 g of iron sulphide is formed. Thus, number of equivalent present in 11.2 g of iron is? tests, examples and also practice UPSC tests.
|
|
Explore Courses for UPSC exam
|
|
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
Follow Us
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup