How many grams of aluminum in required to produce 17.5 g of hydrogen
1 answer:
Mass of Aluminum = 157.5 g
<h3>Further explanation</h3>
Given
17.5 g of Hydrogen
Required
Mass of Aluminum
Solution
Reaction
2Al + 3H₂SO₄ → Al₂(SO₄)₃ + 3H₂
mol Hydrogen :
= mass : molar mass
= 17.5 g : 2 g/mol
= 8.75
From the equation, mol Al :
= 2/3 x mol H₂
= 2/3 x 8.75
= 5.83
Mass Al :
= 5.83 x 27 g/mol
= 157.5 g
You might be interested in
Answer:
Height in meters = 73000 ÷ 100
(1m =100cm)
= 730m
Hope it helps.
The mass of the blood is 5.8 kg.
<em>V</em> = 5.5 L = 5500 mL
Mass = 5500 mL × (1.06 g/1 mL) = 5800 g = 5.8 kg
Energy helps the moving precess
The answer is 59
the atomic mass is the number at the bottom so you've gotta round it to the nearest whole number<span />
The mass of 2.64 moles of water is 47.56 grams
