You are considering transport of Fe3+ out of a biological cell with a membrane potential of -60 mV. What is the value for delta psi in this case? (Make sure you express this value in proper units, i.e., as you would enter this value into the change in free energy of transport equation.)
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You are considering transport of Fe3+ out of a biological cell with a membrane potential of -60 mV. What is the value for delta psi in this case? (Make sure you express this value in proper units, i.e., as you would enter this value into the change in free energy of transport equation.)
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- One of the important uses of the Nernst equation is in describing the flow of ions across plasma membranes. Ions move under the influence of two forces: the concentration gradient (given in electrical units by the Nernst equation) and the electrical gradient (given by the membrane voltage). This is summarized by Ohms law: Ix=Gx(VmEx) which describes the movement of ion x across the membrane. I is the current in amperes (A); G is the conductance, a measure of the permeability of x, in Siemens (S), which is I/V;Vm is the membrane voltage; and Ex is the equilibrium potential of ion x. Not only does this equation tell how large the current is, but it also tells what direction the current is flowing. By convention, a negative value of the current represents either a positive ion entering the cell or a negative ion leaving the cell. The opposite is true of a positive value of the current. a. Using the following information, calculate the magnitude of Na [ Na+ ]0=145mM,[ Na+ ]i=15mM,Gna+=1nS,Vm=70mV b. Is Na+ entering or leaving the cell? c. Is Na+ moving with or against the concentration gradient? Is it moving with or against the electrical gradient?In the situations described below, what is the free energy change if 1 mole of Na+ is transported across a membrane from a region where the concentration is 48 μM to a region where it is 110 mM? (Assume T=37∘C.) When the transport is opposed by a membrane potential of 70 mV.For a typical vertebrate cell with a membrane potential of −0.070 V (inside negative), what is the free-energy change for transporting 1 mol of Na+ from the cell into the blood at 37 °C? Assume the concentration of Na+ insidethe cell is 12 mM and in blood plasma it is 145 mM.
- In the situations described below, what is the free energy change if 1 mole of Na+ is transported across a membrane from a region where the concentration is 48 μM to a region where it is 110 mM? (Assume T=37∘C.) In the absence of a membrane potential.In the following situations, what is the free energy change if 1 mole of Na+is transported across a membrane from a region where the concentration is1 μM to a region where it is 100 mM?(Assume T = 37 °C.) (a) In the absence of a membrane potential. (b) When the transport is opposed by a membrane potential of 70 mV. (c) In each case, will hydrolysis of 1 mole of ATP suffice to drive the transport of 1 mole of ion, assuming pH 7.4 and the following cytoplasmic concentrations: ATP = 4.60 mM, Pi = 5.10 mM, ADP = 310 μM?Calculate the equilibrium membrane potentials to be expected across a membrane at 37 ∘C, with a NaCl concentration of 0.50M on the "right side" and 0.08 M on the "left side", given the following conditions. In each case, state which side is (+) and which is (−). Membrane permeable only to Cl−.
- 1. (a) In class thus far, we have focused our membrane transport energetics discussions on the transfer of K+ ions. Of course, in the cell there are other ions that contribute to the overall resting membrane potential (Autotal). To estimate the overall resting membrane potential for the predominant ions present in the cell, we must first calculate the individual resting membrane potential. Using the Nernst equation discussed in class, and the values provided below, calculate A for each ion. lon K+ Na+ Ca²+ CI- [ion] outside cell 6 mM 145 mM 4 mM 90 mM [ion] inside cell 145mM 8 mM 0.001 mM 6 mMIn considering active transport by Na + -K + -ATPase at body temperature (37 o C), 3 Na+ are pumped out of the cell and 2 K + are pumped in for each ATP that is hydrolyzed to ADP + P i . Given that underyour experimental conditions, the DG for ATP hydrolysis is -10 kcal/mol, and that V is -60 mV, and that the pump maintains the internal Na + at 10mM, external Na + at 120 mM, internal K + at 120 mM and external K + at 8mM, what is the efficiency of the pump (i.e., what fraction of the energy available from ATP hydrolysis is required to drive transport at the provided levels)?Calculate the change in Gibbs free energy for transport of Ca2+ from outside to inside the cell. The extracellular Ca2+ concentration is 135 uM, and the intracellular Ca2+ concentration is 98 uM. The membrane potential is -22 mV and the temperature is 37°C. O. -5.1 kJ/mol O 1.2 kJ/mol -410 kJ/mol 3.4 kJ/mol
- The sarcoplasmic reticulum Ca2+-ATPase, pumps 2 mol Ca2+ out of sarcomeres per mol ATP hydrolyzed. Given the following steady-state concentrations and a membrane potential of 67 mV (inside negative), calculate ΔG for the following active transport process at 37 ∘C and pH=7.4:2Ca2+(in)+ATP+H2O→2Ca2+(out)+ADP+Pi+H+You have a semi permeable membrane with a membrane potential of -90mV. You also have two ions that are both permeable to the membrane, Na and Cl. Na has a concentration of 10mM inside the membrane and 120mM outside the membrane. Cl has a concentration of 1.5mM inside the membrane and 77.5mM outside the membrane. Use the nernst equation to calculate the electrochemical equilibrium of both ions, and show in which direction the netflux would be for each ion.Consider the transport of K+ ions from a surrounding fluid (where [K + ] = 30 mM) into a cell (where [K + ] = 420 mM) where the membrane electrical potential is -0.15 V. Is this process favorable?