Question

If 45.3 g of AgNO₃ react with 28.6 g of H₂SO‚„ according to the unbalanced equation below, what is the mass in grams of Ag₂SO‚„ that could be formed?

AgNO₃(aq) + H₂SO‚„(aq) → Ag₂SO‚„(s) + HNO₃(aq)

Answer 1

To determine the mass of Ag₂SO₄ that could be formed, we need to use the given masses of AgNO₃ and H₂SO₄ and convert them to moles using their respective molar masses. From the balanced equation, we know that the mole ratio between AgNO₃ and Ag₂SO₄ is 1:1.

Step-by-step explanation:

To determine the mass of Ag₂SO₄ that could be formed, we need to use the given masses of AgNO₃ and H₂SO₄ and convert them to moles using their respective molar masses. From the balanced equation, we know that the mole ratio between AgNO₃ and Ag₂SO₄ is 1:1. So, if we have 45.3 g of AgNO₃, we can calculate the moles of Ag₂SO₄ formed. Similarly, if we have 28.6 g of H₂SO₄, we can calculate the moles of Ag₂SO₄ formed. The smaller value of moles obtained from both calculations is the limiting reactant, and we can use this value to calculate the mass of Ag₂SO₄ formed.

Let's calculate the moles of Ag₂SO₄ formed:

1. Find the moles of AgNO₃: