The following concentrations were obtained for the formation of NH3 from N2 and H2 at equilibrium at 500K. [N2] = 1.5 × 10–2M. [H2] = 3.0 ×10–2 M and [NH3] = 1.2 ×10–2M. Calculate equilibrium constant.

Papers Sign In Request access

Free previous-year papers & practice for JEE, NEET and CBSE Boards.

Papers Privacy Terms Contact

Papers Sign In Request access

Free previous-year papers & practice for JEE, NEET and CBSE Boards.

Papers Privacy Terms Contact

Equilibrium Constants Kc and Kp | PadhAiPro

Question

TextEquilibrium Constants Kc and Kp

Similar Questions

At equilibrium, the concentrations of N2=3.0 × 10–3M, O2 = 4.2 × 10–3M and NO= 2.8 × 10–3M in a sealed vessel at 800K. What will be Kc for the reaction N2(g) + O2(g) 2NO(g)

TextEquilibrium Constants Kc and Kp

PCl5, PCl3 and Cl2 are at equilibrium at 500 K and having concentration 1.59M PCl3, 1.59M Cl2 and 1.41 M PCl5. Calculate Kc for the reaction, PCl5 PCl3 + Cl2

TextEquilibrium Constants Kc and Kp

For the equilibrium, 2NOCl(g) 2NO(g) + Cl2(g) the value of the equilibrium constant, Kc is 3.75 × 10–6 at 1069 K. Calculate the Kp for the reaction at this temperature?

TextEquilibrium Constants Kc and Kp

13.8g of N2O4 was placed in a 1L reaction vessel at 400K and allowed to attain equilibrium N2O4 (g) 2NO2 (g). The total pressure at equilbrium was found to be 9.15 bar. Calculate Kc, Kp and partial pressure at equilibrium.

TextEquilibrium Constants Kc and Kp

What is Kc for the following equilibrium when the equilibrium concentration of each substance is: [SO2]= 0.60M, [O2] = 0.82M and [SO3] = 1.90M ? 2SO2(g) + O2(g) 2SO3(g)

TextEquilibrium Constants Kc and Kp

At a certain temperature and total pressure of 105Pa, iodine vapour contains 40% by volume of I atoms I2 (g) 2I (g). Calculate Kp for the equilibrium.

TextEquilibrium Constants Kc and Kp