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polet [3.4K]
3 years ago
11

Two reactions and their equilibrium constants are given. A + 2 B − ⇀ ↽ − 2 C K 1 = 2.37 2 C − ⇀ ↽ − D K 2 = 0.170 Calculate the

value of the equilibrium constant for the reaction D − ⇀ ↽ − A + 2 B .
Chemistry
1 answer:
Marta_Voda [28]3 years ago
7 0

<u>Answer:</u> The value of K_c for the net reaction is 13.94

<u>Explanation:</u>

The given chemical equations follows:

<u>Equation 1:</u>  A+2B\xrightarrow[]{K_1} 2C

<u>Equation 2:</u>  2C\xrightarrow[]{K_2} D

The net equation follows:

D\xrightarrow[]{K_c} A+2B

As, the net reaction is the result of the addition of first equation and the reverse of second equation. So, the equilibrium constant for the net reaction will be the multiplication of first equilibrium constant and the inverse of second equilibrium constant.

The value of equilibrium constant for net reaction is:

K_c=K_1\times \frac{1}{K_2}

We are given:

K_1=2.37

K_2=0.170

Putting values in above equation, we get:

K_c=2.37\times \frac{1}{0.170}=13.94

Hence, the value of K_c for the net reaction is 13.94

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1.The chemical element being the main component of air (it occupies 78% of its volume),

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1) The main component of air that makes up 78% of the air is Nitrogen.

2) The simplest saturated hydrocarbon is the first member of the alkane family, Methane.

3) Two amino acids combine by forming peptide bonds between the carboxyl group of one amino acid and the amino group of another through dehydration synthesis (loss of 1 molecule of water). Hence, the result of the combination of two amino acids are called Dipeptides.

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