While elements and compounds can both be classified as pure substances because they have distinct properties and composition, __
2 answers:
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Answer: The formula of the hydrated alumina is
Explanation:
Decomposition of hydrated alumina is given by:
Molar mass of = 101.96 g/mol
According to stoichiometry:
(101.96+18x) g of decomposes to give 101.96 g of
Thus 5.000 g of
decomposes to give=
of H_2O
But it is given 5.000 g of a sample of hydrated salt was found to contain 2.6763 g of unhydrated salt
Thus we can equate the two equations:
Thus the formula of the hydrated alumina is
Answer:
10 g H₂SO₄
General Formulas and Concepts:
<u>Chemistry - Stoichiometry</u>
- Reading a Periodic Table
- Using Dimensional Analysis
Explanation:
<u>Step 1: Define</u>
Given: 8 g SO₃
RxN: SO₃ + H₂O → H₂SO₄
<u>Step 2: Identify Conversions</u>
Molar Mass of S - 32.07 g/mol
Molar Mass of O - 16.00 g/mol
Molar Mass of H - 1.01 g/mol
Molar Mass of SO₃ - 32.07 + 3(16.00) = 80.07 g/mol
Molar mass of H₂SO₄ - 2(1.01) + 32.07 + 4(16.00) = 98.09 g/mol
<u>Step 3: Stoichiometry</u>
<u /> = 9.80042 g H₂SO₄
<u>Step 4: Check</u>
<em>We are given 1 sig fig. Follow sig fig rules and round.</em>
9.80042 g H₂SO₄ ≈ 10 g H₂SO₄