Chemistry homework

These are a portion of the questions that are needed to be answered. If you decided to complete this assignment I will screenshot and send the remaining 9 questions.1. The equilibrium constant KP for the reaction is 203 at a certain temperature. CalculatePO2ifPNO = 0.411 atm and PNO2 = 0.385 atm.2NO2(g)⇆ 2NO(g) O2(g) PO2 = atm2. Enter your answer in the provided box. For the reaction N2(g) 3H2(g)⇆ 2NH3(g) KP is 0.000817 at 683°C.What is Kc for the reaction? Kc =3. A reaction vessel contains NH3, N2, and H2 at equilibrium at a certain temperature. The equilibrium concentrations are [N2] = 0.41 M, [H2] = 1.26 M, and [NH3] = 0.40 M.Calculate the equilibrium constant, Kc, if the reaction is represented as (1/2)N2(g) (3/2)H2(g) ⇌ NH3(g)4. Ammonium carbamate, NH4CO2NH2,decomposes as follows: NH4CO2NH2(s) ⇆ 2NH3(g) CO2(g) Starting with only the solid, it is found that at 40°C the total gas pressure(NH3 and CO2) is 0.263 atm.Calculate the equilibrium constant KP5. Enter your answer in the provided box.A 2.180 mole quantity of NOCl was initially placed in a1.150 L reaction chamber at 400°C. After equilibrium was established,it was found that 28.60 percent of the NOCl has dissociated:2NOCl(g) ⇆ 2NO(g) Cl2(g)Calculate the equilibrium constant Kc for the reaction.6. At 1000 K, a sample of pure NO2 gas decomposes:2NO2(g) ⇌ 2NO(g) O2(g)The equilibrium constant, KP, is 158. Analysis shows that the partial pressure of O2 is 0.43 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture.13/05/202015chemistry