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Consider the equilibrium system: N2O4(g) + 2 NO2(g) for which Kp = 0.1134 at 25 °C and A Hº = 58.03 kJ/mol. Assume that 1 mole of N204 and 2 moles of NO2 are introduced into a 5.0 liter container. What will be the equilibrium value of [N204]? O 0.928 M 0.379 M 0.0822 M 0.358 M 0.042 M
QUESTION 10 Consider the reaction: 2 NO2(g) = N204(8) AG° = -5.40 kl.mol-1 If NO2 = 0.25 atm and N204 = 0.60 atm, what is A G of the system at 25°C? O A. 2.0 x 102J/mol OB.5.6 kJ/mol O C.-5.4 kJ/mol o D.-4.9 kJ/mol
Arrange the following gases in order of decreasing standard molar entropy: N204(9), NO(g), NO2(g). Select one: O a. N204> NO > NOZ O b. N204 > NO2 > NO O C. NO2 > NO > N20. O d. NO > NO2 > N204 e. NO > N204 > NO2 Which of the following reactions will shift to the left if the volume is decreased? Select one: H2 (8) + Cl2 (8) DIL 2 HCI (8) OD b. 2 SO3 (8)...
Consider the decomposition of N204(g) into NO2(g). N204(g) = 2 NO2(g) kp = 47.9 at 400 K Suppose that 1.00 atm of N204 decomposes and reaches equilibrium at 400 K. Determine the partial pressure of NO2 at equilibrium. 1.96 atm 0.922 atm 1.92 atm 0.960 atm 0.979 atm
5. The equilibrium constant K for the dissociation of N204(g) to NO2(g) is 1700 at 500 K. If AH is 56.8 kJ/mol for this reaction, what will be the value of K at 300 K? (a) 132x106 (b) 1.11 x 104 (c) 0.188 (d) 15.5 (e) .54 x 107
5. The equilibrium constant K for the dissociation of N204(g) to NO2(g) is 1700 at 500 K. If AH is 56.8 kJ/mol for this reaction, what will be the value of...
16. The standard molar free energies of formation of NO2(g) and N204(g) at 25°C are 51.840 and 98.035 kJ/mol, respectively. What is the value of Kp (in atm) for the reaction written as follows at 25°C? A) 6.24 x 10" B) 1.00 C) 9.76 D) 4.38 x 10-36 E) 7.99 x 109
What is AS for the reaction SO2(g) + NO2(g) + S03(g) + NO(g? Substance S'(J/K.mol) SO2(9) 248.5 256.2 NO(g) 210.6 NO2() 240.5 SO3(g) (8 00:51:01 eBook Multiple Choice 0 O 53.6 J/K mol 0 -53.6 J/K mol 0 -22.2 J/K.mol 0 474.8 J/K. mol
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...
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
problem #9 Calculate the equilibrium constant for the following reaction at 25°C. 2H2(g) + O2(g) 2H20cv) Given the following standard free-energy: H2O , -237.2 KJ/mol at 25°C. Problem #10. Given the following data at 25°C: substance sº (J/mol.K) AH', (KJ/mol) 240.45, 33.8 304.33 9.66 NO 249) N2O160) (a) Calculate the value of A Gº for the following reaction at 25°C: 2 NO2(9) N20 (9) (b) Is the formation of NO a spontaneous process at 25°C and standard-state conditions? (a) What...