For which reaction does Kp = Kc? A. 2 NazO2(s) + 2 CO2(g) = 2 Na,CO3(s) + O2(g) B. 2 NiO(s) + CO(g) = Ni(s) + CO2(g) C. NH,NO3(s) = N20(g) + 2 H2O(g)

4) At high temperatures nitrogen (N₂) and oxygen (O₂) will react to form NO. N₂(g) + O₂(g) 2 NO(g) The value for the equilibrium constant for reaction 4.1 is Kc = 2.7 x 10-¹7 at some temperature T. A system initially has [N₂] = 0.0800 M and [0₂] = 0.0500 M. There is no NO initially present in the system. Find the value for [NO] that will be present at equilibrium. (4.1)

The equilibrium constant for the reaction                         2 N2(g) + 5 O2(g)  ⇆  2 N2O5(g) was measured at two temperatures: Temperature, K Kp 343 2.5x10−8 944 7.6x10−6   What is ΔHo for the reaction (in kJ/mol)?

Calculate Kc for the following equilibrium: 2SO2(g) + O2(g) ⇌ 2SO3(g);            Kp = 2.5 × 1010 at 4.5 × 102 K.

You are given the following:   H2 (g) + Br2 (g) 2 HBr (g) Kp = 7.9 x 1011                            H2 (g) 2 H (g) Kp = 4.8 x 10-41                                         Br2 (g) 2 Br (g) Kp = 2.2 x 10-15 What is Kp for the reaction shown below?                                H (g) +  Br (g)   HBr (g) Kp = ?

At 773 °C, a mixture of CO(g), H2(g), and CH3OH(g) was allowed to come to equilibrium. The concentrations were determined to be: [CO] = 0.105 M, [H2] = 0.250 M, [CH3OH] = 0.00261 M. Calculate K. for the reaction CO(g) + 2H2(g) CH3OH(g) Kc = %3D