1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Leokris [45]
3 years ago
14

Gastric juice is made up of substances secreted from parietal cells, chief cells, and mucous-secreting cells. The cells secrete

HCl, proteolytic enzyme zymogens, mucin, and intrinsic factor. The pH of gastric juice is acidic, between 1-3. If the pH of gastric juice is 2.1, what is the amount of energy (?G) required for the transport of hydrogen ions from a cell (internal pH of 7.4) into the stomach lumen? Assume that the potential difference across the membrane separating the cell and the interior of the stomach is �60.0 mV (inside of cells negative relative to the lumen of the stomach).
Assume that the temperature is 37 �C.

The Faraday constant is 96.5 kJ�V�1�mol�1 and the gas constant is 8.314� 10�3 kJ�mol�1�K�1. Express your answer in kJ/mol.
Chemistry
1 answer:
neonofarm [45]3 years ago
5 0

Answer:

The amount of energy required to transport hydrogen ions from a cell into the stomach is 37.26KJ/mol.

Explanation:

The free change for the process can be written in terms of its equilibrium constant as:

ΔG° = -RTInK_(eq)

where:

R= universal gas constant

T= temperature

K_eq= equilibrum constant for the process

Similarly, free energy change and cell potentia; are related to each other as follows;

ΔG= -nFE°

from above;

F = faraday's constant

n = number of electrons exchanged in the process; and  

E = standard cell potential

∴ The amount of energy required for transport of hydrogen ions from a cell into stomach lumen can be calculated as:

ΔG° = -RTInK_(eq)

where;

[texK_eq[/tex]=\frac{[H^+]_(cell)}{[H^+(stomach lumen)]}

For transport of ions to an internal pH of 7.4, the transport taking place can be given as:

H^+_{inside} ⇒ H^+_{outside}

Equilibrum constant for the transport is given as:

K_{eq}=\frac{[H^+]_{outside}}{[H^+]_{inside}}

=\frac{[H^+]_{cell}}{[H^+]_{stomach lumen}}

[H^+]_{cell}= 10⁻⁷⁴

=3.98 * 10⁻⁸M

[H^+]_{stomach lumen} = 10⁻²¹

=7.94 * 10⁻³M

Hence;

K_{eq}=\frac{[H^+]_{cell}}{[H^+]_{stomachlumen}}

=\frac{3.98*10^{-8}}{7.94*10{-3}}

= 5.012 × 10⁻⁶

Furthermore, free energy change for this reaction is related to the equilibrium concentration given as:

ΔG° = -RTInK_(eq)

If temperature T= 37° C ; in kelvin

=37° C + 273.15K

=310.15K; and

R-= 8.314 j/mol/k

substituting the values into the equation we have;

ΔG₁ = -(8.314J/mol/K)(310.15)TIn(5.0126*10^{-6})

= 31467.93Jmol⁻¹

≅ 31.47KJmol⁻¹

If the potential difference across the cell membrane= 60.0mV.

Energy required to cross the cell membrane will be:

ΔG₂ = -nFE°_{membrane}

ΔG₂ = -(1 mol)(96.5KJ/mol/V)(60*10^{-3})

= 5.79KJ

Therefore, for one mole of electron transfer across the membrane; the energy required is 5.79KJmol⁻¹

Now, we  can calculate the total amount of energyy required to transport H⁺ ions across the membrane:

Δ G_{total} = G_{1}+G_{2}

= (31.47+5.79) KJmol⁻¹

= 37.26KJmol⁻¹

We can therefore conclude that;

   The amount of energy required to transport ions from cell to stomach lumen is 37.26KJmol⁻¹

You might be interested in
From where do the gems used in Jewlery come? A. they are mettallic ore B.they are nonmettallic silicates C. they are mettallic m
mixas84 [53]
The answer is D, because gems are usually not mettallic
6 0
3 years ago
Read 2 more answers
Please help me thank you so much <3
aleksandr82 [10.1K]

A i dolnt reaally know but yeh

6 0
2 years ago
Read 2 more answers
Consider the following elementary reaction:
Fudgin [204]

Explanation:

The equation is given as;

N2O(g) ⇄ N2(g) +  O(g)

k₁ = Forward reaction

k₋₁ = Reverse Reaction

Equilibrium concentration (K) = k₁ / k₋₁

K = \frac{[N2O] }{[N2] [ O]}

5 0
2 years ago
How many atoms are in HCOOH₂?
zavuch27 [327]

Answer:

11 atoms I think

Explanation:

4 0
3 years ago
Lecture 19 Equilibrium II Worksheet 1)The equilibrium constant, K c , is 9.8 x 10 5 for H 2 (g) + S (s) H 2 S (g). a.Find the re
Strike441 [17]

Answer:

a) Qc = 0.6338

b) Qc < Kc ⇒ the reaction proceeds to the right, towards the products.

Explanation:

  • H2(g) + S(s) ↔ H2S(g)

∴ Kc = 9.8 E5 = [H2S] / [H2]

a) reaction quotient, Q:

∴ Qc = [H2S] / [H2] = (0.483 M)/(0.762 M) = 0.6338

b) the process is not established equilibrium: Qc < Kc

⇒ The reaction evolves to the right, towards the products

6 0
3 years ago
Read 2 more answers
Other questions:
  • 20 points
    9·1 answer
  • How is a bears fur related to homeostasis?please help. HW
    9·1 answer
  • Assuming the metals lose all their valence electrons and the nonmetals gain electrons to complete the s-p subshells, which listi
    13·1 answer
  • What is the final volume of NaOH solution prepared from 100.0 mL of 0.500 M NaOH if you wanted the final concentration to be 0.1
    9·1 answer
  • Temperature, density, and pressure ______________ (increases, decreases) as depth ____________ (increases, decreases).
    10·2 answers
  • Elements are simple ___
    15·1 answer
  • Which equation would be used to calculate the rate constant from initial<br> concentrations?
    15·2 answers
  • If 60. liters of hydrogen gas at 546 K is cooled to 273 K at constant pressure, the new volume of the gas would be
    12·1 answer
  • Imagine that you and your friend are at the beach. You have your chairs and umbrella set up in the perfect spot near the water s
    7·1 answer
  • If the pressure of the gas is doubled while the volume is held constant, what happens to its temperature?.
    5·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!