Mass of Aluminum= 8.829 g
<h3>Further explanation</h3>
Given
Reaction
2Al + 6HCl → 2AlCl₃ + 3H₂
Required
mass of Aluminum
Solution
At STP, 1 mol gas = 22.4 L
For 11 L of Hydrogen :
= 11 : 22.4
= 0.491
From equation, mol ratio Al : H₂ = 2 : 3, so mol Al :
= 2/3 x mol H₂
= 2/3 x 0.491
= 0.327
Mass Aluminum(Ar=27 g/mol) :
= 0.327 mol x 27 g/mol
= 8.829 g
Answer: first blank is heating second blank is pressure i think but i know that its NOT freezing
Explanation:
I did it and got it right
Answer:

Explanation:
<u>1. Energy to heat the liquid water from 55ºC to 100ºC</u>


<u>2. Energy to change the liquid to steam at 100ºC</u>

- n = 10.1g / 18.015g/mol = 0.5606mol

<u>3. Total energy</u>

Hello!
At
Standard Pressure and Temperature, an ideal gas has a molar density of
0,04464 mol/L.So, we need to apply a simple conversion factor to calculate the density of Sulfur Dioxide using the molar mass of Sulfur Dioxide.

So, the Density of Sulfur Dioxide (SO₂) at STP is
2,8599 g/LHave a nice day!