a. For the reaction: COC₁₂harrCO(g) + Cl2(g), the value of theequilibrium constant, Kc, is 8.1 × 10*. If the initial concentration ofCOCI, is 0.85 molar, find the equilibrium concentrations of all species. bThe reaction: NO2(g) + NO(g) harr N2O(g) + O2(g) has anequilibrium constant, Kp of 0.914. If at some point in time, the partialpressures of both N20 and 0₂ are both 0.425atm and NO2 and NO areboth 0.200atm, find the partial pressures of all gases at equilibrium. c.For the reaction: CO + Cl₂harr COCI₂, the value of the equilibriumconstant, Kc, is 1240. If the initial concentrations of CO and Cl₂ areboth 0.800 molar find the concentrations of all species at equilibrium.

a. For the reaction: COC₁₂harrCO(g) + Cl2(g), the value of the equilibrium constant, Kc, is 8.1 × 10*. If the initial concentration of CoCl2 is 0.85 molar, find the equilibrium concentrations of all species. E The reaction: NO2(g) + NO(g) harr N2O(g) + O2(g) has an equilibrium constant, Kp of 0.914. If at some point in time, the partial pressures of both NO and O2 are both 0.425atm and NO2 and NO are both 0.200atm, find the partial pressures of all gases at equilibrium. c. For the reaction: CO + Cl₂harrCOC₁₂, the value of the equilibrium constant, Kc, is 1240. If the initial concentrations of CO and Cl₂ are both 0.800 molar find the concentrations of all species at equilibrium.

a. For the reaction: COC₁₂harrCO(g) + Cl2(g), the value of the equilibrium constant, Kc, is 8.1 × 10*. If the initial concentration of CoCl2 is 0.85 molar, find the equilibrium concentrations of all species. E The reaction: NO2(g) + NO(g) harr N2O(g) + O2(g) has an equilibrium constant, Kp of 0.914. If at some point in time, the partial pressures of both NO and O2 are both 0.425atm and NO2 and NO are both 0.200atm, find the partial pressures of all gases at equilibrium. c. For the reaction: CO + Cl₂harrCOC₁₂, the value of the equilibrium constant, Kc, is 1240. If the initial concentrations of CO and Cl₂ are both 0.800 molar find the concentrations of all species at equilibrium.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.40PAE: Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that...

See similar textbooks

Similar questions

Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?
What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N2 and O2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
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?