+ Calculating Equilibrium ConstantsThe equilibrium constant, K, of a reaction at a particulartemperature is determined by the concentrations orpressures of the reactants and products at equilibrium.For a gaseous reaction with the general formaA + bB cC + dD=the K, and K₂ expressions are given by[C][D]d[A]a[B]"Kc =KeKp=(Pc) (Pb)(PA)" (PB)The subscript c or p indicates whether K is expressedin terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any puresolids or liquids that may be involved since theircomposition does not change throughout the reaction.The standard state of a pure substance is the puresubstance itself, and although the quantity may changethe sample remain pure. The constant value isincorporated into the value of K, and does not need tobe accounted for separately.Part APhosgene (carbonyl chloride), COC1₂, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene canbe produced by reacting carbon monoxide and chlorine gas at high temperatures:CO(g) + Cl₂ (g) = COCl₂ (g)Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 452 °C. At equilibrium, the concentrations weremeasured and the following results obtained:What is the equilibrium constant, Kp, of this reaction?Express your answer numerically.▸ View Available Hint(s)Kp =SubmitIVE ΑΣΦPrevious Answers******GasCOCl₂| COC1,35 of 43?Review | Constants | Periodic TablePartial Pressure(atm)0.9001.300.120 The equilibrium constant, K, of a reaction at a particulartemperature is determined by the concentrations orpressures of the reactants and products at equilibrium.For a gaseous reaction with the general formaA + bB =cC + dDthe K and K, expressions are given byKc =[C]c[D]d[A]ª[B]b(Pc) (Pb)(PA)" (PB)KpThe subscript c or p indicates whether K is expressedin terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any puresolids or liquids that may be involved since theircomposition does not change throughout the reaction.The standard state of a pure substance is the puresubstance itself, and although the quantity may changethe sample remain pure. The constant value isincorporated into the value of K, and does not need tobe count separately.X Incorrect; Try Again; 5 attempts remainingDeriving concentrations from dataIn Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will begiven initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrationsbefore you can apply the formula for K.Part BThe following reaction was performed in a sealed vessel at 740 °C:H₂(g) + I2(g) = 2HI(g)Initially, only H₂ and I₂ were present at concentrations of [H₂] = 3.00M and [12] = 2.15M. The equilibrium concentration of I2 is0.0700 M. What is the equilibrium constant, Kc, for the reaction at this temperature?Express your answer numerically.► View Available Hint(s)Kc =SubmitIVE ΑΣΦ1?

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Part A Phosgene (carbonyl chloride), COCI₂, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g) + Cl₂(g) = COC1₂(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 452 °C. At equilibrium, the concentrations were measured and the following results obtained: What is the equilibrium constant, Kp. of this reaction? Express your answer numerically. ▸ View Available Hint(s) Kp = Submit ΨΕ ΑΣΦΑ → Previous Answers Gas CO Cl₂ | COC, BO ? Partial Pressure (atm) 0.900 1.30 0.120

Part A Phosgene (carbonyl chloride), COCI₂, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g) + Cl₂(g) = COC1₂(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 452 °C. At equilibrium, the concentrations were measured and the following results obtained: What is the equilibrium constant, Kp. of this reaction? Express your answer numerically. ▸ View Available Hint(s) Kp = Submit ΨΕ ΑΣΦΑ → Previous Answers Gas CO Cl₂ | COC, BO ? Partial Pressure (atm) 0.900 1.30 0.120

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 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...

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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?
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?
Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was injected into a 5.0-L container at 2500 K, at which the equilibrium constant is 3.6 X 10-?. What was the composition of the reaction mixture at equilibrium? l'he 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?
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?
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?
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
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.
For the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.
1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 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?
The equilibrium between nitrogen monoxide, oxygen, and nitrogen dioxide may be expressed in the equation 2NO(g)+O2(g)2NO(g). Write the equilibrium constant expression for this equation. Then express the same equilibrium in at least two other ways, and write the equilibrium constant expression for each. Are the constants numerically equal? Cite some evidence to support your answer. Nitrogen monoxide and oxygen, both colorless gases, react to form reddish-brown nitrogen dioxide.
The equilibrium constant Kc, for the reaction 2 NOCI(g) 2 NO(g) + Cl2(g) is 3.9 103 at 300 C. A mixture contains the gases at the following concentrations: [NOCl] = 5.0 103 mol/L, [NO] = 2.5 103 mol/L, and [Cl2] = 2.0 103 mol/L. Is the reaction at equilibrium at 300 C? If not, in which direction does the reaction proceed to come to equilibrium?
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?