The following diagram represents the reaction of A_2 (dark spheres) with B_2 (li

Question

The following diagram represents the reaction of A_2 (dark spheres) with B_2 (light spheres) Write a balanced equation for the reaction, and circle the species in your equation that is the limiting reactant. How many moles of product can be made from 1.0 mol of A_2 and 1.0 mol of B_2? Box (a) represents 1.0 mL of a solution of molecules at a given concentration. Circle the box (b. c. or d) that represents 1.0 mL of the solution that results after (a) has been diluted by doubling the volume of the solvent.

Explanation / Answer

If we count there are 6 B2 and 4 A2 in the left side diagram and on the product side we can see 2 A2 unreacted and 4 AB3 molecules. From this we can say that B2 are completely consumed and 2 A2 remains unreacted.

We can write balance chemical equation as follows,

4A2 + 6B2 à 4AB3 + 2A2

OR

2A2 + 6B2 à 4AB3; A2 + 3B3à AB3

From this we can say that B2 is a limiting reagent because it got completely consumed in the reaction.

If we see the stoichiometry of reaction we can see that to form 1 mole of product we need 1 mole of A2 and 3 moles of B3.

Since B2 is limiting reagent and 3B2= 1AB3

1.0mol of B2 = 1/3 mol of AB3

Question 8) It is given that box A contains 1ml of solution of certain concentration. If dilute the solution with 1ml water number of mole will be half as that of before.

Previously 1ml= 12 moles after dilution it will be 7 moles = 1ml.

SO, option B is correct.

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