For the reaction: 2 NO2 (g) à N2O4(g) DS0 = -175.5 J/K, DH0=-57.2 kJ
(1) The DG0 is _______ kJ at 325 Celsius.
(2) The reaction is ____ at 325 Celsius. A. for Spontaneous B. nonspontaneous
(3) Would this reaction be spontaneous at___? A. all temperatures B. low temperature C. high temp D. never
(4) Based on your answer of DG0 obtained above, solve for DG if [NO2] = 8.50 atm and [N2O4] = 0.00100 atm. Please have three significant figures and with no units for your
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For the reaction: 2 NO2 (g) à N2O4(g) DS0 = -175.5 J/K, DH0=-57.2 kJ (1) The...
For the reaction: 2 NO2 (g) à N2O4(g) DS0 = -175.5 J/K, DH0=-57.2 kJ (1) The DG0 is _______ kJ at 325 Celsius. Please have one decimal place for your answer (no unit). For example, you can input 100.0 (2) The reaction is ____ at 325 Celsius. A. for Spontaneous B. nonspontaneous Please input letter "A" or letter "B". (3) Would this reaction be spontaneous at___? A. all temperatures B. low temperature C. high temp D. never Please input a letter (A, or B, or...
Thursday Worksheet #13 ve for the K of this reaction at 325 °Celsius. uestions 1 through 5 deal with the reaction: 2 NO2(g) → N204g). 2 Given the above information, solve for the AGº of the reaction at 325 °Celsius and when AH = -57.2 kJ/mol and AS = -175.5 J/(mol-K) determine whether it is spontaneous initially 0.100 atm of NC K you solve for i . Would this reaction be spontaneous at: all temperatures, low temp.
Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K. ______ kJ (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.45 atm and 1.55 atm, respectively. _____ kJ
Consider the reaction 2 NO2(g) →N2O4(g) .(a) Using ΔGfN2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K.kJ(b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.25 atm and 1.30 atm, respectively.kJ
15. Consider the reaction 2 NO2(g) N2O4(g) . (a) Using Gf N2O4(g) = 97.79 kJ/mol and Gf NO2(g) = 51.3 kJ/mol, calculate G° at 298 K. kJ (b) Calculate G at 298 K if the partial pressures of NO2 and N2O4 are 0.35 atm and 1.60 atm, respectively. kJ 16. Consider the reaction given below. H2(g) + F2(g) 2 HF(g) (a) Using thermodynamic data from the course website, calculate G° at 298 K. kJ (b) Calculate G at 298 K...
Find ΔrG for reaction (in kJ mol-1) at 298 K? 2 NO2 (g) ⇌ N2O4 (g) Given Conditions: Pressure: NO2 = 1.25 bar Pressure: N2O4 = 0.65 bar N2O4(g) --
For the dimerization of nitrogen dioxide, ΔG° = −4.7 kJ at 25°C. 2 NO2(g) ⟶ N2O4(g) Calculate ΔG for this reaction if the partial pressures of NO2 and N2O4 are both 0.38 atm. (R = 8.31 × 10−3 kJ/K) a. -10.86 kJ b. -11.36 kJ c. -15.12 kJ d. -11.07 kJ e. -7.10 kJ
What is the ΔrG° for the following reaction (in kJ mol-1)? 2 NO2 (g) ⇌N2O4 (g) To solve, use Appendix II in your textbook (containing standard Gibbs energies of formation) and use the method of Gibbs energy of formation.
The rate of the reaction: CO (g) + NO2 (g) à CO2 (g) + NO (g) was measured at several temperatures, and the following data were collected: Temp (oC) K (M-1s-1) 35 0.184 45 0.322 Using this data determine the value of Ea (energy of activation)
The Kc for the reaction at 298 K is given N2O4(g) ⇋ 2 NO2(g) Kc = 5.9 × 10–3 What is the Kc for the following reaction? ½ N2O4(g) ⇋ NO2(g) Kc = ?