Dissolving silver in concentrated sulfuric acid produced 0.56 liters of sulfur dioxide.

Dissolving silver in concentrated sulfuric acid produced 0.56 liters of sulfur dioxide. Determine the mass of silver taken for the reaction.

Let’s implement the solution:
1. According to the condition of the problem, we compose the equation:
X g -? V = 0.56 l;
2Ag + 2H2SO4 (conc.) = SO2 + AgSO4 + 2H2O – OBP, sulfur dioxide is evolved;
2. We make calculations:
M (Ag) = 107.8 g / mol.
3. Proportions:
1 mole of gas at normal level – 22.4 liters;
X mol (SO2) -0.56 L. hence, X mol (SO2) = 1 * 0.56 / 22.4 = 0.025 mol;
X mol (Ag) – 0.025 mol (SO2);
-2 mol – 1 mol from here, X mol (SO2) = 2 * 0.025 / 1 = 0.05 mol.
4. Find the mass Ag:
m (Ag) = Y * M = 0.05 * 107.8 = 5.39 g.
Answer: to carry out the process, you need silver weighing 5.39 g.