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Anna11 [10]
2 years ago
6

Consider the reaction below.

Chemistry
1 answer:
Luba_88 [7]2 years ago
4 0
Hey there!

I attached a screenshot of my chemistry notes from this year on equilibrium constants in particular. Feel free to reference this in the future if you wish. 

Based on the information in my attachment, you could construct your constant like this:

K_{eq} =  \frac{[CaO][CO_{2}]}{[CaCO_{3}]}

I don't think it matters which order your reactants or products are in as long as you have them on the top and bottom where they need to be, so your answer will be B. 

Hope this helped you out! :-)

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Let's use Boyle's Law here. P1*V1 = P2*V2
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P1 = 900.mmHg
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What is the molar solubility of MgF2 in a 0.36 M Mg(NO3)2 solution? For MgF2, Ksp = 8.4 × 10^–8
Valentin [98]

Answer:

2.4 × 10⁻⁴ M

Explanation:

Step 1: Calculate the concentration of Mg²⁺ coming from Mg(NO₃)₂

Mg(NO₃)₂ is a strong electrolyte and the molar ratio of Mg(NO₃)₂ to Mg²⁺ is 1:1. The initial molar concentration of Mg²⁺ is 1/1 × 0.36 M = 0.36 M.

Step 2: Make an ICE chart for the solution of MgF₂

        MgF₂(s) ⇄ Mg²⁺(aq) + 2 F⁻(aq)

I                           0.36             0

C                           +S             +2S

E                         0.36+S         2S

The solubility product constant is:

Ksp = [Mg²⁺] × [F⁻]² = (0.36+S) × (2S)²

Since S <<< 0.36, 0.36+S ≈ 0.36.

Ksp = 0.36 × 4S² = 8.4 × 10⁻⁸

S = 2.4 × 10⁻⁴ M

7 0
3 years ago
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