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Alex787 [66]
4 years ago
5

The equilibrium constant, Kc, for the reaction N2O4 (g) ⇄ 2NO2 (g) is 0.211 at 100°C. If the equilibrium concentration of N2O4 i

s 0.00251 M, calculate the equilibrium concentration of NO2. View Available Hint(s) The equilibrium constant, Kc, for the reaction N2O4 (g) ⇄ 2NO2 (g) is 0.211 at 100°C. If the equilibrium concentration of N2O4 is 0.00251 M, calculate the equilibrium concentration of NO2. 2.65 × 10-4 M 0.0230 M 2.99 × 10-5 M 5.30 × 10-4 M
Chemistry
1 answer:
julia-pushkina [17]4 years ago
7 0

Answer:

The concentration of NO₂ is 0,0230M

Explanation:

The equilibrium constant, kc, express the ratio in equilibrium between products and reactants. For the reaction:

N₂O₄(g) ⇄ 2NO₂ (g) <em>kc = 0.211 at 100°C</em>

kc = \frac{[NO_{2}]^2}{[N_{2}O_{4}]}

In equilibrium:

0,211 = \frac{[NO_{2}]^2}{[0,00251]}

5,2961x10⁻⁴ = [NO₂]²

<em>0,0230 M = [NO₂]</em>

<em></em>

I hope it helps

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Nucleophilicity is a kinetic property. A higher nucleophilicity indicates that the nucleophile will easily donate its electrons
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The rate constant (K) is related to activation energy (Ea), frequency factor (A) and temperature (T) in Kelvin by the equation

R = molar gas constant

K = A(e^(-Ea/RT))

Taking natural log of both sides

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In K = (-Ea/R)(1/T) + In A

Comparing this to the equation of a straight line; y = mx + c

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K = (3.54 × (10^14))(e^(-91454/(8.314×298.15))) = 0.0336/s

QED!

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