Question:
36 g of A reacts with 54 g of B to form AB\(_2\), if the molar mass of A and B is respectively 60 and 80, then choose the correct option from the following.
36 g of A reacts with 54 g of B to form AB\(_2\), if the molar mass of A and B is respectively 60 and 80, then choose the correct option from the following.
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To determine the limiting reagent, calculate the number of moles of each reactant and compare the ratios based on the balanced equation.
Updated On: Mar 25, 2026
- Limiting Reagent is A
- 90 g of AB\(_2\) formed
- Limiting Reagent is B
- 50 g of AB\(_2\) formed
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The Correct Option is C
Solution and Explanation
Step 1: Calculate the number of moles of A and B.
The number of moles of A: \[ \frac{36}{60} = 0.6 \, \text{mol}. \] The number of moles of B: \[ \frac{54}{80} = 0.675 \, \text{mol}. \] Step 2: Use stoichiometry.
The reaction between A and B is: \[ A + B \rightarrow AB_2. \] From the stoichiometry, 1 mole of A reacts with 1 mole of B to form 1 mole of AB\(_2\). Therefore, A is the limiting reagent because there are fewer moles of A than B. Step 3: Conclusion.
Since A is the limiting reagent, it will determine the amount of AB\(_2\) formed. Final Answer: \[ \boxed{\text{Limiting Reagent is B}}. \]
The number of moles of A: \[ \frac{36}{60} = 0.6 \, \text{mol}. \] The number of moles of B: \[ \frac{54}{80} = 0.675 \, \text{mol}. \] Step 2: Use stoichiometry.
The reaction between A and B is: \[ A + B \rightarrow AB_2. \] From the stoichiometry, 1 mole of A reacts with 1 mole of B to form 1 mole of AB\(_2\). Therefore, A is the limiting reagent because there are fewer moles of A than B. Step 3: Conclusion.
Since A is the limiting reagent, it will determine the amount of AB\(_2\) formed. Final Answer: \[ \boxed{\text{Limiting Reagent is B}}. \]
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