Carbon monoxide is a colorless, odorless gas that binds irreversibly to hemoglobin in our blood, causing suffocation and death. CO is formed during incomplete combustion of carbon. One way to represent this equilibrium is: ? C(s) + 1/2O₂(g) CO(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) 2 C(s) + O₂(g) 2 2C0(g) K₁ = K² 2) 200(g) 22 C(s) + O₂(g) K₂ = 1/K 3) CO(g) 2 C(s) + 1/2O₂(g) K3 = (1/K)² Drag and drop your selection from the following list to complete the answer: K² 1/K (1/K)²

2. The compound NOCl decomposes to nitric oxide and chlorine according to the following equation: 2 NOCl (g) → 2 NO (g) + Cl2 (g) Suppose that 0.810 mol NOCl is placed in a 4.00-L flask at a given temperature. When equilibrium has been established, it is found that the concentration of Cl2 is 0.0105 M. Calculate the equilibrium constant for this reaction.

Consider the following reaction: 2 AB(g) = 2 A(g) + B2(g) The reaction is allowed to proceed until equilibrium is reached, and the final concentrations are: [AB] = 0.041 M [A] = 0.061 M [B2] = 0.030 M %3D %3D %3D Calculate the value of the equilibrium constant, K. Enter the numerical value using 2 significant figures.

At a certain temperature, the equilibrium constant K for the following reaction is 0.0087: NO₂(g) + CO(g) → NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 29. L reaction vessel is filled with 0.27 mol of NO₂ and 0.27 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. NO(g) + CO₂(g) NO₂(g) +CO(g) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(g)+2CO(g) 2NO(g)+2CO₂(g) There will be very little NO₂ and Co. There will be very little NO and CO₂. Neither of the above is true. K = 0 0 0 x10 X ?

A student ran the following reaction in the laboratory at 696 K: 2HI(g) H2(g) + I2(g) When he introduced HI(g) at a pressure of 3.40 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of HI(g) to be 2.68 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp =

O KINETICS AND EQUILIBRIUM Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 380.: NO,(8) + CO(3) = NO(g) + CO,(3) Use this information to complete the following table. Suppose a 16. L reaction vessel is filled with 1.4 mol of NO, and 1.4 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little No, and CO. O There will be very little NO and CO,. O Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] NO(9)+CO,(9) NO,(9)+CO(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] %3D 3 NO,(9)+3CO(g) 3 NO(g)+3CO,(9) 1L Explanation Check III

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.

When 0.16 mol of O2 gas and excess graphite were placed in a 2.00-L container and come to equilibrium, the concentration of CO gas was 0.088 0.024 M. What is the equilibrium constant, Kc, for this reaction at this temperature? Please report 4 decimal places, without units. C(s) + O2(g) ⟷ 2CO(g)

The equilibrium constant for the following reaction is 49 at 450 °C. If 0.22 mole of I2 , 0.22 mole of H2 , and 0.66 mole of HI were put into an evacuated 1.00-liter container, would the system be at equilibrium? If not, what must occur to establish equilibrium? H2 (g) + I2 (g) = 2HI (g)