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. Calculate
PO2
if
PNO = 0.411 atm and PNO2 = 0.385 atm.
2NO2(g) 2NO(g) + O2(g) PO2 = atm
2. 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 KP
5. Enter your answer in the provided box.
A 2.180 mole quantity of NOCl was initially placed in a
1.150 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.
