Given the following reactions, (1) 1/2 N2(g) + 1/2 O2(g) ⇌ NO(g) Kc = 4.8×10^−10 (2) 2 NO(g) + O2(g) ⇌ 2 NO2(g) Kc = 9.1× 10^4 calculate Kc for the reaction below. (3) 2 NO2(g) ⇌ N2(g) + 2 O2(g) Kc = ???
Given the following reactions, (1) 1/2 N2(g) + 1/2 O2(g) ⇌ NO(g) Kc = 4.8×10^−10 (2)...
14. In which of the following reactions will Kc = Ko? ooo 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H2O(g) 2 SO3(g) + 2 NO(g) = 2 SO2(g) + 2 NO2(g) 4 N2(g) + 2 O2(g) = 4 N2O(g) 6 SO2(g) + 3 O2(g) = 6 SO3(g) None of the above reactions have Kc = Kp.
Given the following data at a certain temperature 2N2(g) + O2(g) ? 2N2O(g) N2O4(g) ? 2 NO2(g) 1?2 N2(g) + O2(g) ? NO2(g) Kc=1.2x10-35 ; Kc = 4.6 x 10-3 ; Kc = 4.1 x 10-9 Calculate Kc for the reaction between one mole of dinitrogen oxide gas and oxygen gas to give dinitrogen tetroxide gas.
calculate the equalibrium constant kc for the reaction N2(g)+O2(g)+Br2(g) ---> <--- 2NOBr(g) given the following data: NO(g)+1/2Br(g)---> <---NOBr(g) Kc=1.44 2NO2(g)---> <--- N2(g) +O2(g) Kc=2.1x10^30
1. Which of the following processes is exothermic, given the following: N2(g) + 2 O2(g) + N2O4(1) AH = 9.67 kJ/mol N2(g) + 2 O2(g) + 2 NO2(g) AH = 67.70 kJ/mol A) 2 N2(g) + 4 O2(g) + 2 N204(1) B) 12 N2(g) + O2(g) → % N204(1) C) N2O4(1) + N2(g) + 2 O2(g) D) 2 N2(g) + 4 O2(g) + 2 NO2(g) + N204(1) E) 2 N2(g) + 4 O2(g) → 4NO2(g)
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K (a) What is the value of Kc for the reaction 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) at the same temperature? (b) What is the value of Kc for the reaction 1/2 N2(g) + 1/2 O2(g) equilibrium reaction arrow NO(g) at the same temperature? (c) Does the equilibrium in (a) favor the reactant or the products? reactant products (d) Does the equilibrium in...
Given the following data: () Cu (s) O2 (g)CuO (s) () N2 (g) + 02 (g)NO2 (g) H'--157 kJ AHo+33 kJ calculate AH for the reaction below using Hess' Law. 4 Cu (s) 2 NO2 (g)4 CuO (s) N2 (g)
5. Given the following chemical equilibria, N2(g) + O2(g) = 2 NO(g) N2(g) + 3 H2(g) = 2 NH3(g) H2(g) + 1/2 O2(g) =H2O(g) Determine the method used to calculate the equilibrium constant for the reaction below. 4 NH3(g) + 5 O2(g) = 4 NO(g) + 6 H2O(g) K
A. Based on this question: The reaction between nitrogen and oxygen is given below: N2(g) + O2(g) +2 NO(g) We therefore know that which of the following reactions can also occur? Check which reaction below can occur based on the reaction between nitrogen and oxygen given at N2(g) + O2(g) +2 NO(g) 2 NO(g) + O2(g) 2 NO2(g) 2 NO(g) N2(g) + O2(g) 2 NO2(g) 2 NO(g) + O2(g) or none of the above B. Based on this question: The...
Consider the following data.
2 NO(g) N2(g) + O2(g)
H = -180.7 kJ
2 NO(g) + O2(g) 2 NO2(g)
H = -113.1 kJ
2 N2O(g) 2 N2(g) + O2(g)
H = -163.2 kJ
Use Hess's law to calculate H for the reaction below.
N2O(g) + NO2(g) 3 NO(g)
H =_______ kJ
1. As an EPA scientist studying catalytic converters and urban smog, you want to find Kc for the following reaction: 2 NO2 (g) ⇋ N2(g) + 2 O2(g) Kc = ?? Use the following data to find the unknown Kc: 1/2 N2 (g) + 1/2 O2 (g) ⇋ NO (g) Kc = 0.004 2NO2 (g) ⇋ 2NO (g) + O2 (g) Kc = 0.069 2. A chemical reaction between X2 and Y2 produces XY. All compounds are in a gaseous...