Chemistry · Emf of a Galvanic cell and its measurement, Nernst equation and its applications, relationship between cell potential and Gibbs' energy change
If the pressure of gas is increased from 1atm to 100atm keeping concentration co
If the pressure of \( H_{2} \) gas is increased from 1atm to 100atm keeping \( \boldsymbol{H}^{+} \) concentration constant at \( 1 M, \) the change in reduction potential of hydrogen half cell at \( 25^{\circ} C \) will be:
- A. \( 0.059 V \) \( V \)
- B. \( 0.59 V \)
- C. \( 0.0295 V \)
- D. \( 0.118 V \)
Step-by-step solution
Using Nernst equation: E = E° - (0.059/2) log(P_H2/[H+]^2). With [H+]=1 M constant, at P_H2=1 atm, E=0 V; at P_H2=100 atm, E = -0.0295 log(100) = -0.059 V. Change = -0.059 V, magnitude 0.059 V.
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