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Standard reaction gibbs energy

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Reference no: EM13843023

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?

105_Measuring the voltage-Schematic.jpg

Reference no: EM13843023

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