Question

please answer all or none of thses i need your help are you up for the challenge!!!

For #10-M 3: Consider the gas phase equilibrium, 2 NO2(g)+ 40(g) N20s(g). The enthalpy change for this reaction is -170 kJ and the equilibrium constant is 2.5 at 150 °C. 10. For the above reaction, if N2(g) is added at a constant total pressure of 5 bar, (A) the equilibrium will move to the left and K will decrease the equilibrium will move to the right and K will increase C) the equilibrium will move to the left and K will remain constant (D) the equilibrium will move to the right and K will remain constant 11. For the above reaction, if the temperature is increased, (A) the equilibrium will move to the left and K will decrease (B) the equilibrium will move to the right and K will increase (C) the equilibrium will move to the left and K will remain constant (D) the equilibrium will move to the right and K will remain constant 12. The standard state Gibbs energy change, AG, for the above reaction at 150 °C is approximately: ) -3.2 ม (B) -1.4 kJ (C) -3200 kJ(D) +1.4 kJ 13. What is K for the reaction, 2 N20s(g)4 NO(g) O(g) at 150 °C? (D) 0.63 (A) 6.25 (B) 0.20 (C) 0.16 14. For the gas phase equilibrium, 2A(g) B(g) 2C(g), the equilibrium constant is K- 1x10 If one puts A and B into a vessel with initial pressures, Pm (A) Pmik(B) 3, bar, what is the pressure of C at equililbrium? NOTE: You may assume that very little A and B react. (A) 0.045 bar B) 0.164 b)r(C) 0,082 bar (D) 0063 bar

Answer 1

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PrPd "ThisYUa c.ti on odotn erm/c てステ elecyeass thus the value constant decreage Ptt 0s mole

INC, 5"CD l o loob

pressure 足:24) ב210.OR2 2 0.lCY ber