Answer:
c
Explanation:
use %composition given to calculate emperical 4mular
Answer: The correct option is 3.
Explanation: We are given a compound which is made up of iron and oxygen only. The ratio of the two are given as:
This means that, number of iron ions are 2
Number of oxide ions are 3
From the above information, the formula becomes : 
The valency of iron = 3
Valency of oxide = 2
This compound is named as iron (III) oxide.
Hence, the correct option is 3
Moles of nitrogen = 49.84 / 28 = 1.78
Moles of hydrogen = 10.7 / 2 = 5.35
Molar ratio of nitrogen to hydrogen = 1 : 3
Hydrogen required = 1.78 x 3 = 5.34
Therefore, hydrogen is in excess and nitrogen is the limiting reagent.
Answer:
0.098 moles H₂S
Explanation:
The reaction that takes place is
- 2H₂(g) + S₂(g) ⇄ 2H₂S(g) keq = 7.5
We can express the equilibrium constant as:
- keq = [H₂S]² / [S₂] [H₂]² = 7.5
With the volume we can <u>calculate the equilibrium concentration of H₂</u>:
- [H₂] = 0.072 mol / 2.0 L = 0.036 M
<em>The stoichiometric ratio</em> tells us that <u>the concentration of S₂ is half of the concentration of H₂</u>:
- [S₂] = [H₂] / 2 = 0.036 M / 2 = 0.018 M
Now we <u>can calculate [H₂S]</u>:
- 7.5 = [H₂S]² / (0.018*0.036²)
So 0.013 M is the concentration of H₂S <em>at equilibrium</em>.
- This would amount to (0.013 M * 2.0 L) 0.026 moles of H₂S
- The moles of H₂ at equilibrium are equal to the moles of H₂S that reacted.
Initial moles of H₂S - Moles of H₂S that reacted into H₂ = Moles of H₂S at equilibrium
Initial moles of H₂S - 0.072 mol = 0.026 mol
Initial moles of H₂S = 0.098 moles H₂S
