I₂ (g) + Br₂ (g) ↔ 2IBr (g)
Given is Kc = 280 at 150 degree C.
Kc = [IBr]² / [I₂][Br₂]
Initially [IBr] = 0.45 / 2 = 0.225 M
The actual reaction is:
2IBr ↔ I₂ + Br₂, Kc = 1/280 = 0.00357142
In equilibrium,
[IBr] = 0.225 - 2x
[I₂] = x
[Br₂] = x
By substituting the values we get,
K = [I₂] [Br₂] / [IBr]²
0.00357142 = x×x / (0.225 - 2x)²
√(0.00357142) = x / (0.225 - 2x)
0.0597613 (0.225 - 2x) = x
0.01344 - 2 × 0.0597613x = x
(1 + 2 × 0.0597613)x = 0.01344
x = 0.01344 / (1+2 × 0.0597613)
x = 0.01344 / 1.1195226
x = 0.012005
Substituting the values we get,
IBr = 0.225 - 2 × 0.012005 = 0.17698 M
I₂ = x = 0.012005 M
Br₂ = 0.012005 M
Oak trees:)
Have a great day
If we have 6.68% NaClO, it is the same as saying--> 6.68 grams NaClO= 100 mL of solution. we can use this as a conversion.
800. mL (6.68 mL/ 100 mL)= 53.4 mL
solution = solute + solvent
solute= NaClO
solvent= H2O
solvent= 800-53.4= 747 mL of H2O
so, we you need 53.4 mL of NaClO and 747 mL of water or 53.4 grams of NaClO and 747 mL of water
Answer:
HF
H₂S
H₂CO₃
NH₄⁺
Explanation:
<em>Which acid in each of the following pairs has the stronger conjugate base?</em>
According to Bronsted-Lowry acid-base theory, <em>the weaker an acid, the stronger its conjugate acid</em>. Especially for weak acids, pKa gives information about the strength of such acid. <em>The higher the pKa, the weaker the acid.</em>
<em />
- Of the acids HCl or HF, the one with the stronger conjugate base is HF because it is a weak acid.
- Of the acids H₂S or HNO₂, the one with the stronger conjugate base is H₂S because it is a weaker acid. pKa (H₂S) = 7.04 > pKa (HNO₂) = 3.39
- Of the acids H₂CO₃ or HClO₄, the one with the stronger conjugate base is H₂CO₃ because it is a weak acid.
- Of the acids HF or NH₄⁺, the one with the stronger conjugate base is NH₄⁺ because it is a weaker acid. pKa (HF) = 3.17 < pKa (NH₄⁺) = 9.25
B I hope it’s right I don’t really help a lot but yeah lol
