Consider the following equilibrium at 25°C: 2ICI(g)12(g) + Cl2(g); = 27 kJ, Kp =

Question

Consider the following equilibrium at 25°C: 2ICI(g)12(g) + Cl2(g); = 27 kJ, Kp = 6.2 x 10-6 12. Which of the following would be true if the temperature were increased to 100°c? 1. The value of Kp would increase 2. The concentration of ICI(g) would increase. 3. The partial pressure of I2 would increase. a. 1 only b. 3 only c. 1 and 3 only d. 2 only e. 1 and 2 only 13. One method for the decomposition of carbon dioxide proceeds as follows: 2C02(g)2C00g) +020g); AH= 559 kJ Which of the following changes will cause an increase in the equilibrium concentration of CO? a. adding more Oz to the system b. adding a catalyst c. removing CO2 from the system d. increasing the pressure of the system at constant temperature e. increasing the temperature of the system

Explanation / Answer

13. a. 1 only as the forward reaction is endothermic , increase in temperature increases the equilibrium constant.

14. H3PO4

15. Strong acids will be having weak conjugate bases ,among the acids given H2SO4 and HNO3 are strong acids . among the hypohalous acids HOCl is stronger than HOI. HI is a stronger acid than hypohalous acids.hence HOI will be having the strongest conjugate base.

16. c , one reason why HCl is a stronger acid than HF is that Cl is more electronegative than F, Flourine is more electronegative than chlorine

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