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Paha777 [63]
3 years ago
13

Keq for the reaction below is 2400. If the initial conditions of the reaction are a 1.0 L flask that contains 0.024 mol NO (g),

2.0 mol N2 (g) and 2.6 moles of O2 (g), determine if this reaction is at equilibrium, and, if not which direction it will shift to reach equilibrium.
Chemistry
1 answer:
podryga [215]3 years ago
7 0

Answer:

The answer to your question is it is not at equilibrium, it will move to the products.

Explanation:

Data

Keq = 2400

Volume = 1 L

moles of NO = 0.024

moles of N₂ = 2

moles of O₂ = 2.6

Process

1.- Determine the concentration of reactants and products

[NO] = 0.024 / 1 = 0.024

[N₂] = 2/1 = 2

[O₂] = 2.6/ 1= 2.6

2.- Balanced chemical reaction

                     N₂ + O₂    ⇒   2NO

3.- Write the equation for the equilibrium of this reaction

                     Keq = [NO]²/[N₂][O₂]

- Substitution

                    Keq = [0.024]² / [2][2.6]

-Simplification

                    Keq = 0.000576 / 5.2

-Result

                    Keq = 1.11 x 10⁻⁴

Conclusion

It is not at equilibrium, it will move to the products because the experimental Keq was lower than the Keq theoretical-

                         1.11 x 10⁻⁴ < 2400

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Answer:

The answer to your question is 0.5 moles

Explanation:

Data

moles of Glucose = ?

moles of carbon dioxide = 3

Balanced chemical reaction

                6CO₂  +  6H₂O   ⇒   C₆H₁₂O₆  +  6O₂

Process

To solve this problem, use proportions, and cross multiplication.

Use the coefficients of the balanced equation.

                6 moles of CO₂ ----------------- 1 mol of C₆H₁₂O₆

                3 moles of CO₂ ----------------    x

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-Simplification

                    x = 3/6

-Result

                   x = 0.5 moles of Glucose

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Calculate the number of atoms in 5 moles H₂O.
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Answer:

90.35 × 10²³ atoms

Solution:

1 molecules of H20 contains 3 atoms,.

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