how to calculate kc at a given temperature

4) Write the equilibrium expression, put values in, and solve: Example #8: At 2200 C, Kp = 0.050 for the reaction; What is the partial pressure of NO in equilibrium with N2 and O2 that were placed in a flask at initial pressures of 0.80 and 0.20 atm, respectively? How To Calculate The change in the number of moles of gas molecules for the given equation is, n = number of moles of product - number of moles of reactant. If we know mass, pressure, volume, and temperature of a gas, we can calculate its molar mass by using the ideal gas equation. 5) We can now write the rest of the ICEbox . WebStep 1: Put down for reference the equilibrium equation. A good example of a gaseous homogeneous equilibrium is the conversion of sulphur dioxide to sulphur trioxide at the heart of the Contact Process: Relation Between Kp and Kc 1) The solution technique involves the use of what is most often called an ICEbox. Calculate temperature: T=PVnR. Example of an Equilibrium Constant Calculation. Pressure Constant Kp from Webthe concentration of the product PCl 5(g) will be greater than the concentration of the reactants, so we expect K for this synthesis reaction to be greater than K for the decomposition reaction (the original reaction we were given).. \[K = \dfrac{(a_{H_2O})}{(a_{H_2})}\nonumber\], \[K_p = \dfrac{(P_{H_2O})}{(P_{H_2})}\nonumber\], \[K_p = \dfrac{(0.003)}{(0.013)} = 0.23 \nonumber\]. n = 2 - 2 = 0. G = RT lnKeq. Example . This chemistry video tutorial on chemical equilibrium explains how to calculate kp from kc using a simple formula.my website: How to calculate kc with temperature. AB are the products and (A) (B) are the reagents Example: Calculate the equilibrium constant if the concentrations of Hydrogen gas, carbon (i) oxide, water and carbon (iv) oxide are is 0.040 M, 0.005 M, 0.006 M, 0.080 respectively in the following equation. Where. Step 2: List the initial conditions. At a certain temperature, the solubility of SrCO3 is 7.5 x 10-5 M. Calculate the Ksp for SrCO3. calculate Gibbs free energy Partial Pressures: In a mixture of gases, it is the pressure an individual gas exerts. reaction go almost to completion. x signifies that we know some H2 and I2 get used up, but we don't know how much. T: temperature in Kelvin. A homogeneous equilibrium is one in which everything in the equilibrium mixture is present in the same phase. The equilibrium 3) K Where Calculating Equilibrium Concentration Solution: There is no temperature given, but i was told that it is WebShare calculation and page on. For every one H2 used up, one Br2 is used up also. We can rearrange this equation in terms of moles (n) and then solve for its value. Calculating Equilibrium Concentrations from At a certain temperature, the solubility of SrCO3 is 7.5 x 10-5 M. Calculate the Ksp for SrCO3. Kp = 3.9*10^-2 at 1000 K N2 (g) + 3 H2 (g) <-> The equilibrium constant (Kc) for the reaction . You can determine this by first figuring out which half reactions are most likely to occur in a spontaneous reaction. T - Temperature in Kelvin. At room temperature, this value is approximately 4 for this reaction. Since our calculated value for K is 25, which is larger than K = 0.04 for the original reaction, we are confident our Calculating an Equilibrium Constant Using Partial Pressures Fill in the reaction table below correctly in order to calculate the value of Kc for the reaction A homogeneous equilibrium is one in which everything in the equilibrium mixture is present in the same phase. R f = r b or, kf [a]a [b]b = kb [c]c [d]d. Given that [NOBr] = 0.18 M at equilibrium, select all the options that correctly describe the steps required to calculate Kc for the reaction., R is the gas constant ( 0.08206 atm mol^-1K^-1, ) T is gas temperature in Kelvin. WebH 2 (g) + Br 2 (g) 2HBr (g) Kc = 5.410 18 H 2 (g) + Cl 2 (g) 2HCl (g) Kc = 410 31 H 2 (g) + 12O 2 (g) H 2 O (g) Kc = 2.410 47 This shows that at equilibrium, concentration of the products is very high , i.e. K p is equilibrium constant used when equilibrium concentrations are expressed in atmospheric pressure and K c is equilibrium constant used when equilibrium concentrations are expressed in molarity.. For many general chemical reactions aA + bB cC + dD. Ask question asked 8 years, 5 months ago. \[\ce{N_2 (g) + 3 H_2 (g) \rightleftharpoons 2 NH_3 (g)} \nonumber \]. Pressure Constant Kp from At a certain temperature, the solubility of SrCO3 is 7.5 x 10-5 M. Calculate the Ksp for SrCO3. Let's look at the two "time-frames": INITIALLY or [I] - We are given [N 2] and [H 2]. If H is positive, reaction is endothermic, then: (a) K increases as temperature increases (b) K decreases as temperature decreases If H is negative, reaction is exothermic, then: (a) K decreases as temperature increases Webthe concentration of the product PCl 5(g) will be greater than the concentration of the reactants, so we expect K for this synthesis reaction to be greater than K for the decomposition reaction (the original reaction we were given).. Why? The relationship between Kp and Kc is: \footnotesize K_p = K_c \cdot (R \cdot T)^ {\Delta n} K p = K c (R T)n, where \footnotesize K_p K p is the equilibrium constant in terms of pressure. At equilibrium, rate of the forward reaction = rate of the backward reaction. Pressure Constant Kp from At equilibrium, the concentration of NO is found to be 0.080 M. The value of the equilibrium constant K c for the reaction. Kp = Kc (0.0821 x T) n. In general, we use the symbol K K K K or K c K_\text{c} K c K, start subscript, start text, c, end text, end subscript to represent equilibrium constants. Here is an empty one: The ChemTeam hopes you notice that I, C, E are the first initials of Initial, Change, and Equilibrium. Example #7: Nitrogen and oxygen do not react appreciably at room temperature, as illustrated by our atmosphere. Rank the steps for determining the equilibrium concentrations of the reactants and products in the order that you should carry them out, 1. Recall that the ideal gas equation is given as: PV = nRT. If the reverse reaction is endothermic, a decrease in temperature will cause the system to shift toward the products For example for H2(g) + I2(g) 2HI (g), equilibrium concentrations are: H2 = 0.125 mol dm -3, I2 = 0.020 mol dm-3, HI = 0.500 mol dm-3 Kc = [HI]2 / [H2] [I2] = (0.500)2 / (0.125) x (0.020) = 100 (no units) The steps are as below. Co + h ho + co. WebThe value of the equilibrium constant, K, for a given reaction is dependent on temperature. Then, replace the activities with the partial pressures in the equilibrium constant expression. Remains constant For this, you simply change grams/L to moles/L using the following: The chemical system For convenience, here is the equation again: 9) From there, the solution should be easy. For a chemical reaction, the equilibrium constant can be defined as the ratio between the amount of reactant and the amount of product which is used to determine chemical behaviour. Relationship between Kp and Kc is . How to Calculate Equilibrium \[\ce{2 H_2S (g) \rightleftharpoons 2 H_2 (g) + S_2 (g) } \nonumber\]. the equilibrium constant expression are 1. It's the concentration of the products over reactants, not the reactants over. How To Calculate are the molar concentrations of A, B, C, D (molarity) a, b, c, d, etc. CO + H HO + CO . It would be best if you wrote down For any reversible reaction, there can be constructed an equilibrium constant to describe the equilibrium conditions for that reaction. Kp = (PC)c(PD)d (PA)a(PB)b Partial Pressures: In a mixture of gases, it is the pressure an individual gas exerts. Kp = Kc (R T)n K p = K c ( R T) n. Kp: Pressure Constant. reaction go almost to completion. 0.00512 (0.08206 295) kp = 0.1239 0.124. How to Calculate Equilibrium How to calculate Kp from Kc? Where. It is also directly proportional to moles and temperature. T: temperature in Kelvin. What unit is P in PV nRT? Ab are the products and (a) (b) are the reagents. R: Ideal gas constant. The equilibrium in the hydrolysis of esters. At equilibrium, rate of the forward reaction = rate of the backward reaction. WebFormula to calculate Kp. [PCl3] = 0.00582 M Let's look at the two "time-frames": INITIALLY or [I] - We are given [N 2] and [H 2]. COMPLETE ANSWER: Kc = 1.35 * 10-9 PRACTICE PROBLEMS: Solve the question below involving Kp and Kc. b) Calculate Keq at this temperature and pressure. WebKc= [PCl3] [Cl2] Substituting gives: 1.00 x 16.0 = (x) (x) 3) After suitable manipulation (which you can perform yourself), we arrive at this quadratic equation in standard form: 16x2+ x 1 = 0 4) Using the quadratic formula: x=-b±b2-4⁢a⁢c2⁢a and a = 16, b = 1 and c = 1 we Equilibrium Constant WebKnowing the initial concentration values and equilibrium constant we were able to calculate the equilibrium concentrations for N 2, O 2 and NO. Stack exchange network stack exchange network consists of 180 q&a communities including stack overflow , the largest, most trusted online community for developers to learn, share The value of Q will go down until the value for Kc is arrived at. Example . temperature given Nov 24, 2017. [CO 2] = 0.1908 mol CO 2 /2.00 L = 0.0954 M [H 2] = 0.0454 M [CO] = 0.0046 M [H 2 O] = 0.0046 M Chemistry 12 Tutorial 10 Ksp Calculations How do you find KP from pressure? [Solved!] Webgiven reaction at equilibrium and at a constant temperature. Imagine we have the same reaction at the same temperature \text T T, but this time we measure the following concentrations in a different reaction vessel: Calculating equilibrium constant Kp using This should be pretty easy: The first two values were specified in the problem and the last value ([HI] = 0) come from the fact that the reaction has not yet started, so no HI could have been produced yet. How to Calculate T - Temperature in Kelvin. Calculating equilibrium constant Kp using We know this from the coefficients of the equation. Since K c is being determined, check to see if the given equilibrium amounts are expressed in moles per liter ( molarity ). n = 2 - 2 = 0. The second step is to convert the concentration of the products and the reactants in terms of their Molarity. Remember that solids and pure liquids are ignored. Therefore, Kp = Kc. In this type of problem, the Kc value will be given. The answer obtained in this type of problem CANNOT be negative. In this example they are not; conversion of each is requried. 4) Write the equilibrium constant expression, substitute values into it, and solve: 5) A quadratic equation solver is used. The third step is to form the ICE table and identify what quantities are given and what all needs to be found. We know that the relation between K p and K c is K p = K c (RT) n. 0.00512 (0.08206 295) K p = 0.1239 0.124. Calculating Equilibrium Concentrations from The universal gas constant and temperature of the reaction are already given. For example for H2(g) + I2(g) 2HI (g), equilibrium concentrations are: H2 = 0.125 mol dm -3, I2 = 0.020 mol dm-3, HI = 0.500 mol dm-3 Kc = [HI]2 / [H2] [I2] = (0.500)2 / (0.125) x (0.020) = 100 (no units) The third example will be one in which both roots give positive answers. The equilibrium This is because when calculating activity for a specific reactant or product, the units cancel. At room temperature, this value is approximately 4 for this reaction. aA +bB cC + dD. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Given WebAs long as you keep the temperature the same, whatever proportions of acid and alcohol you mix together, once equilibrium is reached, K c always has the same value. We can check the results by substituting them back into the equilibrium constant expression to see whether they give the same K that we used in the calculation: K = [isobutane] [n-butane] = (0.72 M 0.28 M) = 2.6 This is the same K we were given, so we can be confident of our results. A mixture of 0.200 M NO, 0.050 M H 2, and 0.100 M H 2 O is allowed to reach equilibrium. 4. The concentrations of - do not appear in reaction quotient or equilibrium constant expressions. Co + h ho + co. I think you mean how to calculate change in Gibbs free energy. Notice that moles are given and volume of the container is given. This is the reverse of the last reaction: The K c expression is: WebGiven a reaction , the equilibrium constant , also called or , is defined as follows: R f = r b or, kf [a]a [b]b = kb [c]c [d]d. All reactant and product concentrations are constant at equilibrium. Chapter 14. CHEMICAL EQUILIBRIUM Step 3: The equilibrium constant for the given chemical reaction will be displayed in the output field. Equilibrium Constant How To Calculate Kc With Temperature. K p is equilibrium constant used when equilibrium concentrations are expressed in atmospheric pressure and K c is equilibrium constant used when equilibrium concentrations are expressed in molarity.. For many general chemical reactions aA + bB cC + dD. How to Calculate Equilibrium Constant These will react according to the balanced equation: 2NOBr (g) 2NO (g) + Br2 (g). WebK p = K c ( R T) n g (try to prove this yourself) where n g is number of gaseous products -Number of gaseous reactants. WebKnowing the initial concentration values and equilibrium constant we were able to calculate the equilibrium concentrations for N 2, O 2 and NO. The two is important. Webthe concentration of the product PCl 5(g) will be greater than the concentration of the reactants, so we expect K for this synthesis reaction to be greater than K for the decomposition reaction (the original reaction we were given).. Cindy Wong was a good anatomy student, but she realized she was mixing up the following sound-alike structures in skeletal muscle: myofilaments, myofibrils, fibers, and fascicles. \footnotesize R R is the gas constant. Haiper, Hugo v0.103.0 powered Theme Beautiful Hugo adapted from Beautiful Jekyll Keq - Equilibrium constant. How to Calculate Kc 2) Write the equilibrium constant and put values in: 3) Here comes an important point: we can neglect the '2x' that is in the denominator. R f = r b or, kf [a]a [b]b = kb [c]c [d]d. WebGiven a reaction , the equilibrium constant , also called or , is defined as follows: R f = r b or, kf [a]a [b]b = kb [c]c [d]d. All reactant and product concentrations are constant at equilibrium. Relation Between Kp And Kc Henrys law is written as p = kc, where p is the partial pressure of the gas above the liquid k is Henrys law constant c is the concentration of gas in the liquid Henrys law shows that, as partial pressure decreases, the concentration of gas in the liquid also decreases, which in turn decreases solubility. Henrys law is written as p = kc, where p is the partial pressure of the gas above the liquid k is Henrys law constant c is the concentration of gas in the liquid Henrys law shows that, as partial pressure decreases, the concentration of gas in the liquid also decreases, which in turn decreases solubility. We can check the results by substituting them back into the equilibrium constant expression to see whether they give the same K that we used in the calculation: K = [isobutane] [n-butane] = (0.72 M 0.28 M) = 2.6 This is the same K we were given, so we can be confident of our results. Step 2: List the initial conditions. best if you wrote down the whole calculation method you used. WebK p = K c ( R T) n g (try to prove this yourself) where n g is number of gaseous products -Number of gaseous reactants. The first step is to write down the balanced equation of the chemical reaction. Let's look at the two "time-frames": INITIALLY or [I] - We are given [N 2] and [H 2]. Assume that the temperature remains constant in each case, If the volume of a system initially at equilibrium is decreased the equilibrium will shift in the direction that produces fewer moles of gas I think you mean how to calculate change in Gibbs free energy. There is no temperature given, but i was told that it is still possible Q>1 = The reverse reaction will be more favored and the forward reaction less favored than at standard conditions, If a system at equilibrium is disturbed by a change in concentration the system will shift to the - some of the substance whose concentrations has increased or to - more of a substance whose concentrations has decreased. WebStudy with Quizlet and memorize flashcards containing terms like The equilibrium constant Kc is a special case of the reaction - Qc that occurs when reactant and product concentrations are at their - values, Given the following equilibrium concentrations for the system at a particular temperature, calculate the value of Kc at this temperature The equilibrium constant K c is calculated using molarity and coefficients: K c = [C] c [D] d / [A] a [B] b where: [A], [B], [C], [D] etc. Relationship between Kp and Kc is . Just in case you are not sure, the subscripted zero, as in [H2]o, means the initial concentration. Calculating Equilibrium Concentration Web3. Since our calculated value for K is 25, which is larger than K = 0.04 for the original reaction, we are confident our Kc Q=K The system is at equilibrium and no net reaction occurs WebThis video shows you how to directly calculate Kp from a known Kc value and also how to calculate Kc directly from Kp. How to Calculate Equilibrium Constant At equilibrium in the following reaction at 303 K, the total pressure is 0.016 atm while the partial pressure of \(P_{H_2}\) is found to be 0.013 atm. Construct an equilibrium table and fill in the initial concentrations given Kc The equilibrium concentrations of reactants and products may vary, but the value for K c remains the same. Calculating Equilibrium Concentrations from The relationship between Kp and Kc is: \footnotesize K_p = K_c \cdot (R \cdot T)^ {\Delta n} K p = K c (R T)n, where \footnotesize K_p K p is the equilibrium constant in terms of pressure. \footnotesize R R is the gas constant. What will be observed if the temperature of the system is increased, The equilibrium will shift toward the reactants K_c = 1.1 * 10^(-5) The equilibrium constant is simply a measure of the position of the equilibrium in terms of the concentration of the products and of the reactants in a given equilibrium reaction. Kc: Equilibrium Constant. NO g NO g24() 2 ()ZZXYZZ 2. is 4.63x10-3 at 250C. If the Kc for the chemical equation below is 25 at a temperature of 400K, then what is the Kp? Then, write K (equilibrium constant expression) in terms of activities. The tolerable amount of error has, by general practice, been set at 5%. WebK p And K c. K p And K c are the equilibrium constant of an ideal gaseous mixture. Q=1 = There will be no change in spontaneity from standard conditions WebHow to calculate kc at a given temperature. Since K c is being determined, check to see if the given equilibrium amounts are expressed in moles per liter ( molarity ). Now, I can just see some of you sitting there saying, "Geez, what a wasted paragraph." How To Calculate Kc 3) Write the Kp expression and substitute values: 4) Let's do the algebra leading to a quartic equation: 5) A quartic equation solver to the rescue: 6) The pressure of hydrogen gas at equilibrium was given as '2x:', (144.292 atm) (85.0 L) = (n) (0.08206 L atm / mol K) (825 K), (181.1656 mol) (2.016 g/mol) = 365 g (to three sig figs). Since we are not told anything about NH 3, we assume that initially, [NH 3] = 0. we compare the moles of gas from the product side of the reaction with the moles of gas on the reactant side: Ask question asked 8 years, 5 months ago. Therefore, the Kc is 0.00935. \footnotesize K_c K c is the equilibrium constant in terms of molarity. WebShare calculation and page on. Applying the above formula, we find n is 1. 5. Since we are not told anything about NH 3, we assume that initially, [NH 3] = 0. Calculating equilibrium constant Kp using equilibrium constants Calculations Involving Equilibrium Constant Equation In other words, the equilibrium constant tells you if you should expect the reaction to favor the products or the reactants at a given temperature. WebThis video shows you how to directly calculate Kp from a known Kc value and also how to calculate Kc directly from Kp. Then, Kp and Kc of the equation is calculated as follows, k c = H I 2 H 2 I 2. WebCalculation of Kc or Kp given Kp or Kc . WebTo use the equilibrium constant calculator, follow these steps: Step 1: Enter the reactants, products, and their concentrations in the input fields. \footnotesize K_c K c is the equilibrium constant in terms of molarity. Reactants are in the denominator. The steps are as below. 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