The standard electromotive force (emf) of the cell Pt(s) | H2(g) | HBr(aq) | AgBr(s) | Ag(s) was measured over a range of temperatures, and the data were fitted to the following polynomial:
E0 (V) = 0.07131- 4.99x10-4 (T(K)- 298K)-3.45x10-6 (T(K)- 298K) 2
1. Evaluate the standard reaction Gibbs energy (?rG°) at 298 K.
2. Predict the equilibrium constant, K, from the standard equilibrium constant for the cell reaction Ag+(s) + ½ H2(g) → Ag(s) + H+(aq).
3. Evaluate the standard reaction entropy (?rS°) at 298 K
4. Evaluate the standard reaction enthalpy (?rH°) at 298 K
5. What would be the measured voltage of Schematic A, if R = 1.6111V and M = 1.6021V?
6. The voltmeter, used in Experiment 3, cannot measure voltages below 1 uV and displays 5 significant figures, regardless of the voltage range measured. At room temperature the voltage of battery R and M are 1.6111 V and 1.6021 V, respectively. What is the advantage of measuring the voltage as shown in Schematic A compared to direct measurement of M?
