Question

В 147 гр серной кислоты растворили аммиак сколько г соли получилось​

Answer 1

Дано: m(H2SO4) = 147 г; Найти: m(соли) =?

Решение:  H2SO4 + 2NH3 = (NH4)2SO4 по уравнению реакции

n(H2SO4) = n(соли)   M(H2SO4) = 98 г/моль, М(соли) = 132 г/моль

n(H2SO4) = m/M = 147 / 98 = 1,5 моль

m(соли) = n * M = 1,5 * 132 = 198 г

Answer 2

To determine the amount of salt produced when 147 grams of sulfuric acid (H2SO4) reacts with ammonia (NH3), we first need to write the balanced chemical equation for the reaction:

H2SO4 + 2NH3 → (NH4)2SO4

According to the balanced equation, 1 mole of sulfuric acid (H2SO4) reacts with 2 moles of ammonia (NH3) to produce 1 mole of ammonium sulfate ((NH4)2SO4).

Step 1: Calculate the number of moles of sulfuric acid (H2SO4): Molar mass of H2SO4 = 2 * atomic mass of hydrogen (H) + atomic mass of sulfur (S) + 4 * atomic mass of oxygen (O) Molar mass of H2SO4 = 2 * 1.008 g/mol + 32.06 g/mol + 4 * 16.00 g/mol Molar mass of H2SO4 = 98.08 g/mol

Number of moles of H2SO4 = Mass of H2SO4 / Molar mass of H2SO4 Number of moles of H2SO4 = 147 g / 98.08 g/mol Number of moles of H2SO4 ≈ 1.5 mol

Step 2: Calculate the number of moles of ammonium sulfate ((NH4)2SO4) formed: From the balanced chemical equation, we know that 1 mole of H2SO4 produces 1 mole of (NH4)2SO4.

Number of moles of (NH4)2SO4 = Number of moles of H2SO4 Number of moles of (NH4)2SO4 ≈ 1.5 mol

Step 3: Calculate the mass of ammonium sulfate ((NH4)2SO4) formed: Molar mass of (NH4)2SO4 = 2 * atomic mass of nitrogen (N) + 8 * atomic mass of hydrogen (H) + atomic mass of sulfur (S) + 4 * atomic mass of oxygen (O) Molar mass of (NH4)2SO4 = 2 * 14.01 g/mol + 8 * 1.008 g/mol + 32.06 g/mol + 4 * 16.00 g/mol Molar mass of (NH4)2SO4 = 132.14 g/mol

Mass of (NH4)2SO4 = Number of moles of (NH4)2SO4 * Molar mass of (NH4)2SO4 Mass of (NH4)2SO4 = 1.5 mol * 132.14 g/mol Mass of (NH4)2SO4 ≈ 198.21 g

So, approximately 198.21 grams of ammonium sulfate ((NH4)2SO4) will be produced when 147 grams of sulfuric acid (H2SO4) reacts with ammonia (NH3).