Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached at 298K, PNO = 0.526 atm, PBr2 = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction at 298K. 2NO(g) + Br2 (g) ↔ 2NOBr(g)

4. At 100.°C, Kp = 60.6 for the reaction: 2 NOBr (g) → 2 NO (g) + Br₂ (g). In an experiment, 0.10 atm of each component is placed in a sealed container. Is the mixture at equilibrium? If not, in which direction will the reaction proceed? Show your work to justify your answer.

Consider the reaction N2(g) + O2(g) = 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.28, 0.26, and 0.025 atm, respectively, at 2200°C, what is Kp?

Calcium sulfate decomposes to calcium oxide, sulfur dioxide and oxygen according to this reaction equation: 2CaSO4(s) ⇌ CaO(s) + 2SO2(g) + O2(g) Starting with pure gypsum at 1371 °C in a closed container, the equilibrium system develops a total pressure of 0.089 atm. Calculate Kp for the reaction at 1371 °C.

Consider the following equilibrium process at 686. °℃: CO₂(g) + H₂(g) CO(g) + H₂O(g) The equilibrium concentrations of the reacting species are [CO]=0.0560 M, [H₂] = 0.0400 M, [CO₂]=0.0830 M, and [H₂O]=0.0430 M. Part 1 of 5 Calculate K for the reaction at 686. °C. Round your answer to 3 significant digits. с Kc- Part 2 of 5 x10 If we add CO₂ to increase its concentration to 0.510 M, what will the concentrations of all the gases be when equilibrium is reestablished? Round your answer to 3 significant digits. [CO₂] = M x10 X Ś

Equilibrium mixture in a 2.50 L flask at 250 °C in the reaction PCI3(g) + Cl₂(g) →PCI5(g); It contains 0.105 g PCI5, 0.220 g PCI3, and 2.12 g Cl₂. What is the value of (a) Kc and (b) Kp for this reaction at 250 °C? P: 31 g/mol; CI: 35.5 g/mol

Determine Kp for the chemical equation you have written.

At 2516 °C the equilibrium constant for the reaction: 2 BrCl(g) Br₂(g) + Cl₂(g) is Kp = 0.863. If the initial pressure of BrCl is 0.00277 atm, what are the equilibrium partial pressures of BrCl, Br₂, and Cl₂? p(BrCl) = p(Br₂) = p(Cl₂) =

Consider the following reaction: CO2(g) + C(graphite) = 2 CO(g) A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO. If the equilibrium pressure of CO gas is 0.83 atm, find the equilibrium constant (Kp) for the reaction.

The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K.Calculate Kp for this reaction at this temperature.NH4HS(s) NH3(g) + H2S(g)