Question

The Nernst equation at 20oC is:

Answer 1

Answer:

a. -58 millivolts

Explanation:

The given Nernst equation is:

$E_{ion} = 58 millivolts /z \Big[ log_{10} \Big( \dfrac{[ion]_{out}}{[ion]_{in}}\Big) \Big]}$

The equilibrium potential given by the Nernst equation can be determined by using the formula:

$E_{Cl^-} = \dfrac{2.303*R*T}{ZF} \times log \dfrac{[Cl^-]_{out}} {[Cl^-]_{in}}$

where:

gas constant(R) = 8.314 J/K/mol

Temperature (T) = (20+273)K

= 298K

Faraday constant F = 96485 C/mol

Number of electron on Cl = -1

$E_{Cl^-} = \dfrac{2.303*8.314*298} {(-1)*(96845)} \times log \dfrac{100} {10}$

$E_{Cl^-} = - 0.05814 \ volts$

$\mathsf{E_{Cl^-} = - 0.05814 \times 1000 \ milli volts}$

$\mathsf{E_{Cl^-} \simeq - 58\ milli volts}$