Question

An amount of 1.0 x 10⁻³ moles of Ag and 1.0 x 10⁻³ moles of Cr₄²⁻ combine to form solid Ag₂CrO₄. What is the amount of Ag₂CrO₄ formed?

a. 1.0 x 10⁻³ moles
b. 2.0 x 10⁻³ moles
c. 3.0 x 10⁻³ moles
d. 4.0 x 10⁻³ moles

Answer 1

The correct amount of Ag₂CrO₄ formed when 1.0 x 10⁻³ moles of Ag and CrO₄²⁻ combine is 1.0 x 10⁻³ moles.

Step-by-step explanation:

When 1.0 x 10⁻³ moles of Ag are combined with 1.0 x 10⁻³ moles of CrO₄²⁻, solid Ag₂CrO₄ is formed.

According to the balanced chemical equation, 2 mol of Ag+ reacts with 1 mol of CrO₄²⁻ to form 1 mol of Ag₂CrO₄.

Since the molar ratio of Ag+ to CrO₄²⁻ is 2:1, the limiting reagent in this case would be Ag+. Thus, 1.0 x 10⁻³ moles of CrO₄²⁻ will react with 2 x 1.0 x 10⁻³ moles of Ag+ to produce 1.0 x 10⁻³ moles of Ag₂CrO₄.

Hence, the correct option is (a) 1.0 x 10⁻³ moles of Ag₂CrO₄ formed.