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raketka [301]
3 years ago
6

Each enzyme functions in a different area of the body, but both work to harness the power in carbohydrates and break these compl

ex molecules into simple sugars. Based on the information you have learned about the digestive system, what do you expect to be the optimal pH for the enzymatic action of pancreatic amylase?
Chemistry
2 answers:
mylen [45]3 years ago
7 0
The optimal pH is 6.9. The pancreatic amylase is a hydrolase secreted by the pancreas and will go into the alimentary canal. The working environment has a pH of 6.9. So the optimal pH for the enzyme needs to be 6.9.

Explanation:

The optimum pH scale for the catalyst activity of secretion enzyme ranges from half-dozen to seven. higher than and below this vary, the reaction rate reduces as enzymes get denaturated. The accelerator secretion enzyme is most active at pH scale 6.8.
Human duct gland alpha-amylase. II. Effects of hydrogen ion concentration, substrate and ions on the activity of the protein. refined human duct gland alpha-amylase (alpha-1,4-glucan 4-glucanohydrolase, EC 3.2.1.1) was found to be stable over a large vary of hydrogen ion concentration<span> values (5.0 to 10.5.</span>
Whitepunk [10]3 years ago
5 0
The optimal pH is 6.9. The pancreatic amylase is a hydrolase secreted by pancreas and will go into the alimentary canal. The working environment has a pH of 6.9. So the optimal pH for the enzyme needs to be 6.9.
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Which element glows red when electricity flows through it?
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In thermodynamics, we determine the spontaneity of a reaction by the sign of ΔG. In electrochemistry, spontaneity is determined
faltersainse [42]

<u>Answer:</u>

<u>For A:</u> The standard cell potential of the reaction is 4.4 V

<u>For B:</u> The standard Gibbs free energy of the reaction is -8.50\times 10^5J

<u>For C:</u> The reaction is spontaneous as written.

<u>Explanation:</u>

  • <u>For A:</u>

The given chemical reaction follows:

2Li(s)+Cl_2(g)\rightarrow 2Li^+(aq.)+2Cl^-(aq.)

The given half reaction follows:

<u>Oxidation half reaction:</u>  Li(s)\rightarrow Li^+(aq.)+e^-;E^o_{Li^+/Li}=-3.04V ( × 2)

<u>Reduction half reaction:</u>  Cl_2(g)+2e^-\rightarrow 2Cl^-(aq.);E^o_{Cl_2/2Cl^-}=+1.36V

The substance having highest positive E^o potential will always get reduced and will undergo reduction reaction.

Here, chlorine will undergo reduction reaction will get reduced.

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

To calculate the E^o_{cell} of the reaction, we use the equation:

E^o_{cell}=E^o_{cathode}-E^o_{anode}

E^o_{cell}=1.36-(-3.04)=4.4V

Hence, the standard cell potential of the reaction is 4.4 V

  • <u>For B:</u>

Relationship between standard Gibbs free energy and standard electrode potential follows:

\Delta G^o=-nFE^o_{cell}

where,

n = number of electrons transferred = 2mol\text{ e}^-

F = Faradays constant = 96500J/V.mol\text{ e}^-

E^o_{cell} = standard cell potential = 4.4 V

Putting values in above equation, we get:

\Delta G^o=-2\times 96500\times 4.4=-849200J=-8.50\times 10^5J

Hence, the standard Gibbs free energy of the reaction is -8.50\times 10^5J

  • <u>For C:</u>

For a reaction to be spontaneous, the standard Gibbs free energy change of the reaction must be negative.

From above, the standard Gibbs free energy change of the reaction is coming out to be negative.

Hence, the reaction is spontaneous as written.

7 0
4 years ago
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