<span> A </span>catalyst<span> will </span>appear<span> in the steps of a </span>reaction<span> mechanism, but it will not </span>appear<span> in the overall </span><span>chemical reaction</span>
Best Answer: 4.52 X 10²³ atoms. Use Avogadro's number to multiply 0.750 moles times 6.022 X 10²³
Answer: Option (B) is the correct answer.
Explanation:
Molar mass is defined as the sum of masses of all the atoms present in a compound.
For example, atomic mass of barium is 137.32 g/mol and atomic mass of bromine is 79.90 g/mol.
Therefore, molar mass of 
will be as follows.
Molar mass = atomic mass of Ba + 
= 137.32 g/mol + 
= 297.12 g/mol
Hence, we can conclude that molar mass of [tex]BaBr_{2}[tex] is 297.12 g/mol.
I believe the answer is C
Leftover: approximately 11.73 g of sulfuric acid.
<h3>Explanation</h3>
Which reactant is <em>in excess</em>?
The theoretical yield of water from Al(OH)₃ is lower than that from H₂SO₄. As a result,
- Al(OH)₃ is the limiting reactant.
- H₂SO₄ is in excess.
How many <em>moles</em> of H₂SO₄ is consumed?
Balanced equation:
2 Al(OH)₃ + 3 H₂SO₄ → Al₂(SO₄)₃ + 6 H₂O
Each mole of Al(OH)₃ corresponds to 3/2 moles of H₂SO4. The formula mass of Al(OH)₃ is 78.003 g/mol. There are 15 / 78.003 = 0.19230 moles of Al(OH)₃ in the five grams of Al(OH)₃ available. Al(OH)₃ is in excess, meaning that all 0.19230 moles will be consumed. Accordingly, 0.19230 × 3/2 = 0.28845 moles of H₂SO₄ will be consumed.
How many <em>grams</em> of H₂SO₄ is consumed?
The molar mass of H₂SO₄ is 98.076 g.mol. The mass of 0.28845 moles of H₂SO₄ is 0.28845 × 98.076 = 28.289 g.
How many <em>grams</em> of H₂SO₄ is in excess?
40 grams of sulfuric acid H₂SO₄ is available. 28.289 grams is consumed. The remaining 40 - 28.289 = 11.711 g is in excess. That's closest to the first option: 11.73 g of sulfuric acid.
