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3 years ago

What is one product of a condensation reaction between two amino acids, such as glycine and alanine?

Chemistry

1 answer:

Ipatiy [6.2K]3 years ago

3 0

Answer:

Gly-Ala

(Dipeptide).

Explanation:

A condensation reaction is a reaction in which two molecules combine to form a single molecule with the loss of a small molecule e.g water.

When two amino acids, such as alanine and glycine react, they yield a mixture of dipeptides (via dipeptide bond) and water. That is, The −OH from the carboxyl group (-COOH) of one amino acid combines with a hydrogen atom from the amine group (-NH2) of the other amino acid to produce water.

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The adult blue whale has a lung capacity 5.0\times10^3 5.0 Ã 10 3 l. calculate the mass of air (assume an average molar mass of

Andre45 [30]

For this item, we need to assume that air behaves like that of an ideal gas. Ideal gases follow the ideal gas law which can be written as follow,
PV = nRT
where P is the pressure,
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3 years ago

Before any reaction occurs, the concentration of A in the reaction below is 0.0510 M. What is the equilibrium constant if the co

Lilit [14]

Answer:

0.0119

Explanation:

There was a part missing. I think this is the whole question:

Before any reaction occurs, the concentration of A in the reaction below is 0.0510 M. What is the equilibrium constant if the concentration of A at equilibrium is 0.0153 M?

A (aq) ⇌ 2B (aq) + C(aq)

Remember to use correct significant figures in your answer. Do not include units in your response.

First, we have to make an ICE Chart, which stands for initial, change and equilibrium. We will call "x" unknown concentrations.

A (aq) ⇌ 2B (aq) + C (aq)

I 0.0510 0 0

C -x +2x +x

E 0.0510-x 2x x

Since the concentration at equilibrium of A is 0.0153 M, we get

$0.0510 - x = 0.0153 \\x = 0.0357$

We can use the value of x to calculate the concentrations at equilibrium.

$[A]e = 0.0153 M \\[B]e = 2x = 2(0.0357) = 0.0714 M \\[C]e = x = 0.0357 M \\$

The equilibrium constant, Kc, is the ratio of the equilibrium concentrations of products over the equilibrium concentrations of reactants each raised to the power of their stoichiometric coefficients.

$Kc = \frac{[B]^{2} \times [C]}{[A]} = \frac{0.0714^{2} \times 0.0357}{0.0153} = 0.0119$

The equilibrium constant for this reaction at equilibrium is 0.0119.

You can learn more about equilibrium here: brainly.com/question/4289021

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