An oxygen (0,) molecule is adsorbed onto a small patch of the surface of a catalyst. It's known that the molecule is adsorbed on 1 of 81 possible sites for adsorption (see sketch at right). Calculate the entropy of this system. Round your answer to 3 significant digits, and be sure it has the correct unit symbol. An C at or
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- An adsorption study where RDB (Rhodamine B) molecule was adsorbed byZnCl2 liquid phase and was monitored in the range of 35oC to 60oC. Thecorresponding equilibrium constants are attached as image in a tabular form. Calculate the change of enthalpy and entropy of adsorption process.Assuming that the reaction is spontaneous.Solve for the standard heat of the ff reaction @ 298K.Two helium atoms adsorb to a surface which has 20 sites to which it can adhere. What is the entropy of the system?
- In Experiment 1 we measured the solubility in water of a readily soluble substance at different temperatures and determined four important thermodynamic quantities (ΔH0 = 19.71 ΔG0 = - 4.21 , ΔS0 = 80.22, and K298 = 5.47) for the dissolution process. The same four thermodynamic quantities can be determined for the dissolution of a sparingly soluble substance in water such as benzoic acid, but the numerical values are then quite different and reflect the differentiation between readily and sparingly soluble substances in water. Predict how you expect each of the four thermodynamic quantities for the dissolution of benzoic acid in water will differ from the values you determined for the dissolution process of potassium nitrate. Use for your prediction words like “larger” or “smaller”, “change sign” or “order of magnitude difference” and motivate your prediction in each case. ΔoplosH0: motivation: ΔoplosS0: motivation ΔoplosG0: motivation: K298: motivation:The entropy of reaction at T=198.15K and a pressure of 5 bar.If the adsorption of a gas onto a surface is found, somewhat unusually, to be endothermic, what can be said about the entropy change on adsorption?
- Define and Derive the Nernst EquationIt is found that the energy required to reduce particles from a mean diameter of l.00 cm to 0.300 cm is 11.0 kJ/kg. Estimate the energy requirement to reduce the same particles from a diameter of 0.100 cm to 0.0100 cm. [Note: Use Bond’s Law to solve this problem.]Calculate the standard free energy for the reaction at 340.0°C. (you may use any valid technique - there may be more than one way to do a question like this):
- Consider the reaction in the attached image: a. The standard Gibbs free energy (ΔfG˚) for this reaction (up to two decimal places) is ____________ kJ/mol. b. If the concentration of AMP is adjusted to 1.5M and that of adenosine and phosphate is adjusted to 0.50M, the actual free energy change (ΔG) (up to two decimal places) is equal to ___________ kJ/mol.Can the Nernst equation be used at temperatures other than room temperature?A chart is prepared by plotting In Ksp versus 1/T, using data obtained by performing a lab experiment. Refer to the attached photo for guidance on how to perform these calculations; Equation 5 is particularly useful. A linear fit of the data in the chart yields the equation y = (-4.976x10^3)x+(1.9900x10^1) with an R2 value of 0.9922. Determine the entropy (deltaS in J/K) associated with dissolving KNO3. Answer in scientific notation with appropriate sigfigs.