Please find the thermodynamic data and determine the Kvalue at 25\deg C, 5\deg C, &100\deg C for the formation of aragonite (CaCO3) from Ca²+ ? (aq) and bicarbonate (HCO34Grxn, the 4SRXn, and the 4H\deg rxn. Finally give the K value for each temperature

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Given the following two measurements of the equilibrium constant for a reaction, calculate DH° for the reaction. T,°C K 5.6 x 106 1.3х 109 35.0 54.0 Tvne v Our an swer

calculate Kp and Kc from the delta G for the following reactions at 100 C and determine if this reaction is likely to be spontaneous: 2SO3(g) -- 2SO2(g) + O2(g)

Consider the reactionI2(g) + Cl2(g)2ICl(g)Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.

ment/takeCovalentActivity.do?locator3Dassignment-take Review Topical Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° =-87.9 kJ, and K. = 83.3 , at 500 K: PCI3 (g) + Cl2 (g) PCI5 (g) If the TEMPERATURE on the equilibrium system is suddenly increased: The value ofK. A. Increases B. Decreases C. Remains the same The value of Qe A. Is greater than K. B. Is equal to K. C. Is less than K. The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Cl, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 8 more group attempts remaining Pre 50 hp

Q4. (a) What is Eell for the following unbalanced reaction? Fe (s) + O2 (g) + 2H20 (4) Fe3 (aq) + 40H (aq) (b) Balance the reaction. (c) What is A,G° for the reaction? (d) What are the conditions of the above process?

Calculate the AH°, AS°, and AG° at 298 K for the following reaction: (Use the values found in Thermodynamic Properties to calculate your answers for questions a and b.) Al2O3(s) + 3 C(graphite) + 3 Cl₂(g) → 2 AICI3(s) + 3 CO(g) a) ΔΗο 400-64 kJ/mol b) AS° J/K.mol c) AGO 4.0 ✔ kJ/mol (Determine from the temperature, AH and AS) (d) Is the reaction extensive at standard conditions and 298 K? O Yes O NO 4.0 76.9 -89 (e) Write the expression for K. (Format example: Kp = pHC1² / pH₂. pCl2 would be entered as K_{p} = pHCI^{2}/pH_{2} . pCl_{2}.) Help chemPad X₁X (PCO)³ (pCl₂)3 Greek (PCO)^3/(pCl_2)^3 Your answer provides a different type of equation than was expected. (f) Calculate the value of K at 298 K 2.51e-16 X (Please answer to 3 significant figures.) (g) Estimate the value of K at 600 K. 1 79e-8 Ty (Please answer to 3 significant figures)

Calculate ΔH°, ΔS° and ΔG° for the synthesis of SO3(g) Be sure to use the values provided in this table:  Compound          ΔHf° (kJ/mol)                  S° (J/Kmol)   SO2(g)                   -253                               231 SO3(g)                    -345                                219 O2(g)                          0                                   205 a) give the balance equation for the synthesis of SO3(g) from SO2(g) and O2(g) b) What is ΔH° for this process? c) What is ΔS° for this process? d) What is ΔG° for this process?

The Ostwald process for the commercial production of nitric acid involves three steps. 4 NH3(g) + 5 02(9) 4 NO(g) + 6 H20(g) 2 NO(g) + 02(g) → 2 NO2(g) 3 NO2(g) + H20(1) → 2 HNO3(/) + NO(g) (a) Calculate AH°, AS°, AG°, and K (at 298 K) for each of the three steps in the Ostwald process (see Appendix 4). (Use the values you calculate for AH° and AS° to calculate AG°.) first step second step third step AH° -908 V kJ ΔΗ -112 V kJ AH° -74 kJ AS° 181 V J/K AS° -147 V J/K AS° |-267 V J/K AG° -928 V kJ AG° -70 V kJ AG° 6 x kJ K 0.11 K 1.03 K 0.089 (b) Calculate the equilibrium constant for the first step at 825°C, assuming AH° and AS° do not depend on temperature. 41.45 (c) Is there a thermodynamic reason for the high temperature in the first step assuming standard conditions? O Yes O No Explain. > > > x