CO(g) + H2O(g)CO2(g) + H2(g) Kc = 102 at 500 KA reaction mixture initially contains 0.130 MCO and 0.130 MH2O. What will be the equilibrium concentration of H2O?

7-40 Is there any change in conditions that change the equilibrium constant, K, of a given reaction?

7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.

7-28 When the following reaction reached equilibrium at 325 K, the equilibrium constant was found to be 172. When a sample was taken of the equilibrium mixture, it was found to contain 0.0714 M NO2. What was the equilibrium concentration of N2O4?

The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.

Nitric oxide and bromine at initial partial pressures of 98.4 and 41.3 torr, respectively, were allowed to react at 300. K. At equilibrium the total pressure was 110.5 torr. The reaction is 2NO(g)+Br2(g)2NOBr(g) a. Calculate the value of Kp. b. What would be the partial pressures of all species if NO and Br2, both at an initial partial pressure of 0.30 atm, were allowed to come to equilibrium at this temperature?

7-32 A particular reaction has an equilibrium constant of 1.13 under one set of conditions and an equilibrium constant of 1.72 under a different set of conditions. Which conditions would be more advantageous in an industrial process that sought to obtain the maximum amount of products? Explain.

Write the mathematical expression for the reaction quotient, QC, for each of the following reactions (a) N2(g)+3H2(g)2NH3(g) (b) 4NH3(g)+5O2(g)4NO(g)+6H2O(g) (C) N2O2(g)2NO2(g) (d) CO2(g)+H2CO(g)+H2O(g) (e) NH4CI(s)NH3(g)+HCI(g) (f) 2Pb( NO3)2(s)2PbO(s)+4NO2(g)+O2(g) (g) 2H2(g)+O2(g)2H2O(g) (h) S8(g)8S(g)

Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.

A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?