Lab 1 Postlab - Richard Germade-Craan Chem 1200 The ∆H...

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Richard Germade-Craan Chem 1200 Section 04 Lab 1: Enthalpy and Entropy of Zinc with Copper Sulfate Post Lab Calorimetry: 1. According to the plot, the temperature of the copper sulfate solution before mixing (T i ) was 9.690°C, the maximum temperature of the mixture was 39.969°C. The total change in temperature was 30.279°C. 2. ∆H = + K WT i Tfn = . - ° - + ° - . ° / 3 8 J g 1 C 150 g 30 J C 130 279 C50 g . 159 6095gmol = 18,364.9684 J/mol = 18.364 kJ/mol 3. Electrochemistry: 4. As found by the analysis function in Microlab, the equation for the linear curve fit for the plot is y = -0.0006x + 1.0217 5. 6. ∆S = slope* F = (.0006)(96,500 C/mol) = 57.9 J/K 7. ∆H = y-intercept* F = (1.0217)(96,500 C/mol) = 98,594 J = 98.594 kJ 8. 9. ∆G = ∆H - T∆S = 98,594 J – (25+298.15 K)(57.9 J/K) = 79,883.15 J = 79.883 kJ 10. E = ∆G/-n F = 79,883.15/96,500 = .827 V
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Unformatted text preview: Richard Germade-Craan Chem 1200 Section 04 11. The ∆H value I obtained by the calorimetry equation seems a lot more reasonable than the ∆H I obtained by the electrochemistry equation, which leads me to think that either I did the electrochemistry equation wrong, or that the microlab data wasn’t collected properly. 12. For the calorimetry method, error could have happened during the weighing of the zinc powder. The scale might have been off, I could have read it wrong, or zinc could have fallen during the transfer to the beaker setup. For the electrochemistry method, error could have happened with the sensor if it had not been properly calibrated, or we could have started recording data before the system had reached it’s equilibrium. 13....
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Lab 1 Postlab - Richard Germade-Craan Chem 1200 The ∆H...

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