I can't seem to figure out how to solve this?

Question

If 0.200 moles of AgNO₃ react with 0.155 moles of H₂SO₄ according to this UNBALANCED equation below, what is the mass in grams of Ag₂SO₄ that could be formed? AgNO₃(aq) + H₂SO₄ (aq) → Ag₂SO₄ (s) + HNO₃ (aq)

Answer 1

First, balance the equation ...

2AgNO₃(aq) + H₂SO₄(aq) ==> Ag₂SO₄(s) + 2HNO₃(aq) ... balanced equation

Next, find which reactant is limiting. An easy way to do this is to divide the moles of each reactant by the respective coefficient in the balanced equation and see which value is less.

For AgNO₃: 0.200 moles (÷2->0.100)

For H₂SO₄: 0.155 moles (÷1->0.155)

AgNO₃ is LIMITING since 0.100 is less than 0.155

Finally, use the MOLES of the limiting reactant (0.200 moles) to determine the theoretical yield of Ag₂SO₄. We also need the molar mass of Ag₂SO₄ which is 312 g / mol.

0.200 mol AgNO₃ x 1 mol Ag₂SO₄ / 2 mol AgNO₃ x 312 g Ag₂SO₄ / mol = 31.2 g Ag₂SO₄