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Marianna [84]
3 years ago
13

Draw a Lewis structure for [H3O]+. Show all unshared pairs and the formal charges, if any.

Chemistry
1 answer:
Montano1993 [528]3 years ago
3 0

Answer: Formal Charges: Hydrogen = 0 and Oxygen = +1

Unshared Pair of electrons: Hydrogen = 0 and Oxygen = 2

Explanation:

The attachment below shows the Lewis structure and the calculations

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A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C.
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The equilibrium constant of the reaction is 282. Option D

<h3>What is equilibrium constant?</h3>

The term equilibrium constant refers to the number that often depict how much the process is able to turn the reactants in to products. In other words, if the reactants are readily turned into products, then it follows that the equilibrium constant will be large and positive.

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Concentration of iodine = 1.600 mol/1.000-L =  1.600M

In this case, we must set up the ICE table as shown;

              Br2(g) + I2(g) ↔ 2IBr(g)

I          0.6            1.6           0

C      -x                -x             +2x

E    0.6 - x         1.6 - x       1.190

If 2x = 1.190

x = 1.190/2

x = 0.595

The concentrations at equilibrium are;

[Br2] = 0.6 -  0.595 = 0.005

[I2] =   1.6 - 0.595 = 1.005

Hence;

Kc = [IBr]^2/[Br2] [I2]

Kc = ( 1.190)^2/(0.005) (1.005)

Kc = 282

Learn more about equilibrium constant:brainly.com/question/15118952

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A and B are two imaginary substances. The molecules of substance A have weak electrical forces between them. The
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