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Reil [10]
3 years ago
13

Consider the following reaction: NH4I(s) NH3(g) + HI(g) If a flask maintained at 674 K contains 0.138 moles of NH4I(s) in equili

brium with 4.34×10-2 M NH3(g) and 9.39×10-2 M HI(g), what is the value of the equilbrium constant at 674 K?
Chemistry
1 answer:
xz_007 [3.2K]3 years ago
4 0

Answer:

4.08 × 10⁻³

Explanation:

Step 1: Write the balanced reaction at equilibrium

NH₄I(s) ⇄ NH₃(g) + HI(g)

Step 2: Calculate the equilibrium constant

The equilibrium constant (K) is equal to the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients. Only gases and aqueous species are included.

K = [NH_3] \times [HI] = 4.34 \times 10^{-2}  \times 9.39 \times 10^{-2} = 4.08 \times 10^{-3}

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</span>Na2CO3 would increase by 116.8 / 106 = 1.10 to form 2NaCl.
<span>0.4862 g x 1.10 = 0.515 grams of NaCl.
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K2CO3 + 2Cl- ⇒ 2KCl + CO3^-2 
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<span>2 moles of KCl = 149.1 </span>
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K2CO3 would increase by </span>149.1 /138.2 = 1.079 <span>to form 2KCl
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<span> 0.4862 x 1.079 = 0.5246 g</span>


3 0
3 years ago
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A block of ice has a weight of 35
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Problem 2 - The mass of Earth is 6.0x1024 kg. The mass of a hydrogen atom is
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4 0
3 years ago
Suppose that 273 of a substance displaces 26ml of water what is the substance
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3 0
3 years ago
Determine the pH of the resulting solution if 25 mL of 0.400 M strychnine (C21H22N2O2) is added to 50 mL of 0.200 M HCl? Assume
DIA [1.3K]

Answer:

pH = 4.56

Explanation:

The strychnine reacts with HCl as follows:

C₂₁H₂₂N₂O₂ + HCl ⇄ C₂₁H₂₂N₂O₂H⁺ + Cl⁻

<em />

For strychnine buffer:

pOH = 5.74 + log [C₂₁H₂₂N₂O₂H⁺] / [C₂₁H₂₂N₂O₂]

Initial moles of C₂₁H₂₂N₂O₂ are:

0.025L * (0.400 mol / L) = 0.01 moles C₂₁H₂₂N₂O₂

And of HCl are:

0.05L * (0.200 mol / L) = 0.01 moles HCl

That means after the reaction, you will have just 0.01 moles of C₂₁H₂₂N₂O₂H⁺ in 50mL + 25mL = 0.075L. And molarity is:

[C₂₁H₂₂N₂O₂H⁺] = 0.01 mol / 0.075L = 0.1333M

This conjugate acid, is in equilibrium with water as follows:

C₂₁H₂₂N₂O₂H⁺(aq) + H₂O(l) ⇄ C₂₁H₂₂N₂O₂ + H₃O⁺

<em />

<em>Where Ka = Kw / Kb = 1x10⁻¹⁴ / 1.8x10⁻⁶ = 5.556x10⁻⁹</em>

<em />

Ka is defined as:

Ka = 5.556x10⁻⁹ = [C₂₁H₂₂N₂O₂] [H₃O⁺] / [C₂₁H₂₂N₂O₂H⁺]

In equilibrium, concentrations are:

C₂₁H₂₂N₂O₂ = X

H₃O⁺ = X

C₂₁H₂₂N₂O₂H⁺ = 0.1333M - X

Replacing in Ka expression:

5.556x10⁻⁹ = [X] [X] / [0.1333M - X]

7.39x10⁻¹⁰ - 5.556x10⁻⁹X = X²

7.39x10⁻¹⁰ - 5.556x10⁻⁹X - X² = 0

Solving for X:

X = - 2.72x10⁻⁵M → False solution. There is no negative concentrations

X = 2.72x10⁻⁵M → Right solution.

As H₃O⁺ = X

H₃O⁺ = 2.72x10⁻⁵M

And pH = -log H₃O⁺

<h3>pH = 4.56</h3>
4 0
3 years ago
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