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PSYCHO15rus [73]
2 years ago
11

Use the "x is small" approximation to find the concentration of the products in the following reaction which initially contains

only 0.85 M HCN. Decide whether using the approximation was valid or invalid.HCN(aq) ⇌ H+(aq) + CN−(aq), Kc= 6.17 x 10−10
Chemistry
1 answer:
Mrrafil [7]2 years ago
4 0

Answer:

Concentration of product at equilibrium ;

[H^+]=0.0000229 M

[CN^-]=0.0000229 M

Explanation:

HCN(aq)\rightleftharpoons H^+(aq) + CN^-(aq)

initially

0.85 M        0    0

(0.85-x)M    x      x

The equilibrium constant of reaction = K_c= 6.17\times 10^{-10}

The expression of an equilibrium cannot can be written as:

K_c=\frac{[H^+][CN^-]}{[HCN]}

6.17\times 10^{-10}=\frac{x\times x}{(0.85-x)}

Solving for x:

x = 0.0000229

Concentration of product at equilibrium ;

[H^+]=0.0000229 M

[CN^-]=0.0000229 M

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Answer:

P = 0.0166 mm Hg

Explanation:

To solve this question, we need to use the Clausius Clapeyron equation, which is a commonly used expression to calculate vapour pressure at a given temperature. We have the enthalpy of vaporization of the mercury, so, let's write the equation:

Clausius Clapeyron equation:

Ln (P₂ / P₁) = (-ΔHv / R)(1/T₂ - 1/T₁)    (1)

Where:

R: universal constant of gases (8.314 J / K.mol)

P₂: Vapour pressure at 43°C (or 316 K)

P₁: Pressure of mercury at the boiling point (1 atm)

T₂: temperature at 43 °C

T₁: Boiling point of mercury (357 °C or 630 K)

As we are given the boiling point of the mercury, we can safely assume that the pressure at this point is 1 atm, becuase remember that when a sustance boils, is because it's internal pressure has reached the atmospherical pressure of 1 atm. With this clear, all we just need to do is solve for P₂. We are going to do this very slowly so you can understand the process. First let's replace the given data:

Ln (P₂ / 1) = (-59100 J/mol / 8.314 J / K.mol) (1/316 - 1/630)

Ln P₂ = -7108.49 * (3.16x10⁻³ - 1.59x10⁻³)

Ln P₂ = -7108.49 * (1.51x10⁻³)

Ln P₂ = -10.7338

P₂ = 10⁽⁻¹⁰°⁷³³⁸⁾

P₂ = 2.18x10⁻⁵ atm

We can express this value in mm Hg and it will be:

P₂ = 2.18x10⁻⁵ * 760

<h2>P₂ = 0.0166 mm Hg</h2>

Hope this helps

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n = ??
n = C * V
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Find the molar mass
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Find the mass
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given mass = molar mass * mols
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