Question

How many grams of H2SO4 do I need to use in order to produce 3.01 moles of water? consider the equation. _Ca(OH)2 + _H2SO4 = _CaSO4 + _H20​

Answer 1

Answer:

148 g H₂SO₄

General Formulas and Concepts:

Chemistry - Stoichiometry

• Reading a Periodic Table
• Balancing RxN's
• Using Dimensional Analysis

Explanation:

Step 1: Define

RxN:   Ca(OH)₂ + H₂SO₄ → CaSO₄ + H₂O

Given:   3.01 moles H₂O

Step 2: Balance RxN

Ca(OH)₂ + H₂SO₄ → CaSO₄ + 2H₂O

• Need the same amount of O's and H's on both sides

Step 3: Define conversions

Molar Mass of H - 1.01 g/mol

Molar Mass of S - 32.07 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of H₂SO₄ - 2(1.01) + 32.07 + 4(16.00) = 98.09 g/mol

Step 4: Stoichiometry

$3.01 \ mol \ H_2O(\frac{1 \ mol \ H_2SO_4}{2 \ mol \ H_2O} )(\frac{98.09 \ g \ H_2SO_4}{1 \ mol \ H_2SO_4} )$ = 147.625 g H₂SO₄

Step 5: Check

We are given 3 sig figs. Follow sig fig rules.

147.625 g H₂SO₄ ≈ 148 g H₂SO₄