3. Calculate P [NO]eq, if P [NOCl]eq = 0.60 atm, P [Cl2]eq = 1.50 atm, and Kp = 3.9 × 10-2. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)
3. Calculate P [NO]eq, if P [NOCl]eq = 0.60 atm, P [Cl2]eq = 1.50 atm, and...
Calculate P [NO]eq, if P [NOCl]eq = 0.33 atm, P [Cl2]eq = 0.50 atm, and Kp = 1.9 x 10-2.2 NOCl(g) ?? 2 NO(g) + Cl2(g)13)A) 1.7 atm B) 0.30 atm C) 0.0042 atm D) 0.087 atm E) 0.064 atm
2 NOCl(g) ⇄ 2 NO(g) + Cl2(g) Kp = 7.2× 10-6 1.50 atm of NOCl(g) is placed in a container and the system is allowed to reach equilibrium. Calculate the equilibrium pressure of Cl2(g) at equilibrium. 4.8 × 10-2 atm 8.5 × 10-3 atm 3.2 × 10-2 atm 2.4 × 10-2 atm 1.6 × 10-2 atm
6) Calculate the pressures of all species at equilibrium in a mixture of NOCl, NO, and Cl2 produced when a sample of NOCl with an initial pressure of 10.0 atm comes to equilibrium according to this reaction: 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) KP=4.0×10−4
saw an answer posted already, but think it is wrong as they used Kp = [NOCL]^2/ [NO]^2 x [Cl2]. In this question, NOCl is the reactant, and I thought Kp = [products] / [reactants] An evacuated reaction vessel is filled with 3.60 atm of NOCI. When the system reaches equilibrium according to the reaction below, there are 0.160 atm of NOCI. What is Kp for this reaction? 2 NO (g) + Cl2 (g) = 2 NOCI (g)
A mixture of 0.1182 mol of O2, 0.05082 mol of NOCl, 0.1918 mol of NO2, and 0.1196 mol of Cl2 is placed in a 1.0-L steel pressure vessel at 604 K. The following equilibrium is established: 1 O2(g) + 2 NOCl(g) 2 NO2(g) + 1 Cl2(g) At equilibrium 0.03160 mol of NOCl is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of O2, NOCl, NO2, and Cl2. Peq(O2) = . Peq(NOCl) = . Peq(NO2) = . Peq(Cl2)...
A 1.90 mole quantity of NOCl was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 22.0 percent of the NOCl had dissociated: 2NOCl(g) 2NO(g) + Cl2(g) Calculate the equilibrium constant Kc for the reaction.
consider following reaction: 2 NO + Cl2⇌ 2 NOCl for which K= 6.25*10^4. Calculate K for the following reaction 6 NOCl⇌ 6 NO + 3 Cl2
The reaction 2 NO+Cl2 2 NOCl is at equilibrium at 25'C when PNo-0.24 atm, Pc 0.61 C12 Poo,-1.35 atm. What is the value of ΔGo for the reaction?
The equilibrium constant, Kc, for the reaction 2 NOCl (g) ⇄ 2 NO (g) + Cl2 (g) is 2.4 x 10-7. What is the equilibrium constant for the reaction Cl2 (g) + 2 NO (g) ⇄ 2 NOCl
Calculate the activation energy for the gas phase reaction: 2 NOCl(g) ® 2 NO(g) + Cl2(g) given the following data: T(K) rate constant (L mol-1s-1) 400 6.95 × 10-4 450 1.98 × 10-2 500 2.92 × 10-1 550 2.60 600 16.3