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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?
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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.
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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?
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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?.
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