Calculate how many grams of potassium sulfate will be released when 4.9 grams of sulfuric acid

Calculate how many grams of potassium sulfate will be released when 4.9 grams of sulfuric acid reacts with potassium hydroxide.

H2SO4 + 2KOH = K2SO4 + 2H2O
According to the periodic table, we determine the molar mass of sulfuric acid: M = 1 * 2 + 32 + 16 * 4 = 98 g / mol. And the molar mass of potassium sulfate: M = 39 * 2 + 32 + 16 * 4 = 174 g / mol.
Let’s find the amount of sulfuric acid: n = m / M = 4.9 g / 98 g / mol = 0.05 mol.
According to the reaction, 1 mol of potassium sulfate is formed from 1 mol of sulfuric acid, which means n (H2SO4) = n (K2SO4) = 0.05 mol.
Find the mass of potassium sulfate: m = n * M = 0.05 mol * 174 g / mol = 8.7 mol.
Answer: m (K2SO4) = 8.7 mol.

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