Chem Mantra

25.4 g of iodine and 14.2g of chlorine are made to react completely to yield a mixture of ICl and \(\mathrm{ICl_3}\) Calcualte the ratio of moles of I...

Posted by Chem Mantra
Solved
Mole conceptBasic stoichiometry, POAC, percent yield & limiting reagentHARDJEE Chemistry
25.4 g of iodine and 14.2g of chlorine are made to react completely to yield a mixture of ICl and \(\mathrm{ICl_3}\) Calcualte the ratio of moles of ICl and \(\mathrm{ICl_3}\) **Options:** - **A.** [object Object] - **B.** [object Object] - **C.** [object Object] - **D.** [object Object] --- **Difficulty:** HARD | **Chapter:** Mole concept | **Topic:** Basic stoichiometry, POAC, percent yield & limiting reagent

Official Solution

## ✅ Correct Answer: **A** ### 📖 Detailed Explanation: This question uses stoichiometry and limiting reagent. Write the balanced chemical equation, compute moles of each reactant, identify the limiting reagent, and use stoichiometric ratios (and % yield, if needed) to obtain the answer; this gives option A. --- *This is an official solution provided by Chem Mantra. For more chemistry questions and solutions, explore our [question bank](/courses).*

Solution verified by Chem Mantra faculty

Want More Practice Questions?

Access thousands of JEE Chemistry questions with detailed solutions

Explore CoursesBrowse More Questions

Related Topics

Mole conceptBasic stoichiometry, POAC, percent yield & limiting reagentHARDJEE Chemistry