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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. Therefore, the Kc is 0.00935. T: temperature in Kelvin. A flask initially contained hydrogen sulfide at a pressure of 5.00 atm at 313 K. When the reaction reached equilibrium, the partial pressure of sulfur vapor was found to be 0.15 atm. 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. \(K_{eq}\) does not have units. The equilibrium constant Kc for the reaction shown below is 3.8 x 10-5 at 727C. Solids and pure liquids are omitted. The best way to explain is by example. Calculate all three equilibrium concentrations when Kc = 20.0 and [H2]o = 1.00 M and [Cl2]o = 2.00 M. 4) After suitable manipulation (which you can perform yourself), we arrive at this quadratic equation in standard form: 5) Using the quadratic formula, we obtain: 6) In this problem, note that b equals (60). 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. 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. Finally, substitute the calculated partial pressures into the equation. The Kc was determined in another experiment to be 0.0125. Given that [NOBr] = 0.18 M at equilibrium, select all the options that correctly describe the steps required to calculate Kc for the reaction., If the number of moles of gas is the same for the reactants and products a change in the system volume will not effect the equilibrium position, You are given Kc as well as the initial reactant concentrations for a chemical system at a particular temperature. the whole calculation method you used. WebFormula to calculate Kc. The universal gas constant and temperature of the reaction are already given. This tool calculates the Pressure Constant Kp of a chemical reaction from its Equilibrium Constant 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. According to the ideal gas law, partial pressure is inversely proportional to volume. Then, Kp and Kc of the equation is calculated as follows, k c = H I 2 H 2 I 2. Which best describes the rates of the forward and reverse reactions as the system approaches equilibrium, The rate of the forward reaction increases and the rate of the reverse reaction decreases, Select all the statements that correctly describe what happens when a stress is applied to a system at equilibrium, When stress is applied to a system at equilibrium the system reacts to minimize the effect of the stress It's the concentration of the products over reactants, not the reactants over. The third example will be one in which both roots give positive answers. It is also directly proportional to moles and temperature. Select g in the circuit of the given figure so that the output voltage is 10V10 \mathrm{~V}10V. 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, Match the magnitude of the equilibrium constant Kc with the correct description of the system, Value of the Kc is very large = equilibrium lies to the right, As a rule of thumb an equilibrium constant Kc that has a value less than - is considered small, The equilibrium constant Kc for a particular reaction is equal to 1.22*10^14. WebFormula to calculate Kp. This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here! Other Characteristics of Kc 1) Equilibrium can be approached from either direction. At room temperature, this value is approximately 4 for this reaction. 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. 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. 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. I hope you don't get caught in the same mistake. Tour Start here for a quick overview of the site Help Center Detailed answers to any questions you might have Meta Discuss the workings and policies of this site R is the gas constant ( 0.08206 atm mol^-1K^-1, ) T is gas temperature in Kelvin. 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 Calculate temperature: T=PVnR. In your question, n g = 0 so K p = K c = 2.43 Share Improve this answer Follow edited Nov 10, 2018 at 8:45 answered Nov 10, 2018 at 2:32 user600016 967 1 9 24 Thank you! \[\ce{N_2 (g) + 3 H_2 (g) \rightleftharpoons 2 NH_3 (g)} \nonumber \]. 4) Now, we compare Q to Kc: Is Q greater than, lesser than, or equal to Kc? At a certain temperature, the solubility of SrCO3 is 7.5 x 10-5 M. Calculate the Ksp for SrCO3. Kp = (PC)c(PD)d (PA)a(PB)b Partial Pressures: In a mixture of gases, it is the pressure an individual gas exerts. 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) WebStep 1: Put down for reference the equilibrium equation. Web3. Select the correct expressions for Kc for the reaction, The value of the equilibrium constant K for the forward reaction is - the value of K for the reverse reaction, The value of Kc for a given reaction is the equilibrium constant based on -, The partial pressure of the reactants and products, Select all the statements that correctly describe the equation below, Delta-n indicates the change in the number of moles of gases in the reaction Even if you don't understand why, memorize the idea that the coefficients attach on front of each x. Kp = (PC)c(PD)d (PA)a(PB)b Partial Pressures: In a mixture of gases, it is the pressure an individual gas exerts. Petrucci, et al. 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 WebTo do the calculation you simply plug in the equilibrium concentrations into your expression for Kc. Where. 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 What is the equilibrium constant at the same temperature if delta n is -2 mol gas . 3) K How to calculate kc at a given temperature. reaction go almost to completion. NO g NO g24() 2 ()ZZXYZZ 2. is 4.63x10-3 at 250C. So when calculating \(K_{eq}\), one is working with activity values with no units, which will bring about a \(K_{eq}\) value with no units. T - Temperature in Kelvin. Ask question asked 8 years, 5 months ago. Calculating equilibrium concentrations from a set of initial concentrations takes more calculation steps. WebWrite the equlibrium expression for the reaction system. The equilibrium constant is known as \(K_{eq}\). The positive signifies that more HI is being made as the reaction proceeds on its way to equilibrium. 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. 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. 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).. Initially the concentration of NOCl2 is high and the concentration of NO(g) and Cl2(g) are zero. To do this, we determine if the value we calculated for 2x is less than 5% of the original concentration, the 0.40. The answer is determined to be: at 620 C where K = 1.63 x 103. This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here! Construct an equilibrium table and fill in the initial concentrations given You just plug into the equilibrium expression and solve for Kc. At equilibrium, rate of the forward reaction = rate of the backward reaction. Here is the initial row, filled in: Remember, the last value of zero come from the fact that the reaction has not yet started, so no HBr could have been produced yet. Webgiven reaction at equilibrium and at a constant temperature. For every one H2 used up, one I2 is used up also. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Using the value of x that you calculated determine the equilibrium concentrations of all species, As a reaction proceeds in the forward direction to establish equilibrium, the value of Q -, If a system at equilibrium contains gaseous reactants or products a decrease in the volume of the system will cause the system to shift in the direction the produces - moles of gas, whereas an increase in volume causes a shift in the direction that produces - moles of gas, Match each relationship between Q and K to the correct description of how the reaction will proceed, QK The reaction proceeds towards the reactants, Equilibrium: The Extent of Chemical Reactions, Donald A. McQuarrie, Ethan B Gallogly, Peter A Rock, Ch. Kc=62 of its stoichiometric coefficient, divided by the concentration of each reactant raised to the power of its stoichiometric coefficient. How do i determine the equilibrium concentration given kc and the concentrations of component gases? Relationship between Kp and Kc is . What are the concentrations of all three chemical species after the reaction has come to equilibrium? The steps are as below. Once we get the value for moles, we can then divide the mass of gas by To find , How to calculate Kp from Kc? Why has my pension credit stopped; Use the gas constant that will give for partial pressure units of bar. \footnotesize K_c K c is the equilibrium constant in terms of molarity. The first step is to write down the balanced equation of the chemical reaction. This also messes up a lot of people. Recall that the ideal gas equation is given as: PV = nRT. (a) k increases as temperature increases. . Example #6: 0.850 mol each of N2 and O2 are introduced into a 15.0 L flask and allowed to react at constant temperature. WebStudy with Quizlet and memorize flashcards containing terms like 0.20 mol of NO (g) is placed in a 1-L container with 0.15 mol of Br2 (g). What we do know is that an EQUAL amount of each will be used up. Feb 16, 2014 at 1:11 $begingroup$ i used k. Use the gas constant that will give for partial pressure units of bar. WebCalculation of Kc or Kp given Kp or Kc . C2H4(g)+H2O(g)-->C2H5OH(g) These will react according to the balanced equation: 2NOBr (g) 2NO (g) + Br2 (g). O3(g) = 163.4 What unit is P in PV nRT? n = 2 - 2 = 0. 7) Determine the equilibrium concentrations and then check for correctness by inserting back into the equilibrium expression. R f = r b or, kf [a]a [b]b = kb [c]c [d]d. How to calculate kc with temperature. There is no temperature given, but i was told that it is still possible In this example they are not; conversion of each is requried. Since there are many different types of reversible reactions, there are many different types of equilibrium constants: \[K_p = \dfrac{(P_C)^c(P_D)^d}{(P_A)^a(P_B)^b}\]. That means that all the powers in the There is no temperature given, but i was told that it is Step 3: The equilibrium constant for the given chemical reaction will be displayed in the output field. We can rearrange this equation in terms of moles (n) and then solve for its value. The equilibrium constant (Kc) for the reaction . R is the gas constant ( 0.08206 atm mol^-1K^-1, ) T is gas temperature in Kelvin. At equilibrium in the following reaction at room temperature, the partial pressures of the gases are found to be \(P_{N_2}\) = 0.094 atm, \(P_{H_2}\) = 0.039 atm, and \(P_{NH_3}\) = 0.003 atm. PCl3(g)-->PCl3(g)+Cl2(g) In my classroom, I used to point this out over and over, yet some people seem to never hear. Applying the above formula, we find n is 1. WebKnowing the initial concentration values and equilibrium constant we were able to calculate the equilibrium concentrations for N 2, O 2 and NO. Step 3: List the equilibrium conditions in terms of x. Step 3: The equilibrium constant for the given chemical reaction will be displayed in the output field. Step 3: List the equilibrium conditions in terms of x. This is the one that causes the most difficulty in understanding: The minus sign comes from the fact that the H2 and I2 amounts are going to go down as the reaction proceeds. At equilibrium, the concentration of NO is found to be 0.080 M. The value of the equilibrium constant K c for the reaction. Construct a table like hers. Since we are not told anything about NH 3, we assume that initially, [NH 3] = 0. A good example of a gaseous homogeneous equilibrium is the conversion of sulphur dioxide to sulphur trioxide at the heart of the Contact Process: [c2211c94], Life Insurance Policies: The Amazing Ones With No Medical Exam, Life Insurance Costs and Payouts At Different Ages You Should Know. O2(g) = 0, Select all the statements that correctly describe how an equilibrium system containing gases will respond to changes in volume or pressure. Use the stoichiometry of the balanced chemical equation to define, in terms of x, the amounts of other species consumed or produced in the reaction \[K = \dfrac{(a_{NH_3})^2}{(a_{N_2})(a_{H_2})^3} \nonumber\]. Nov 24, 2017. How to calculate kc with temperature. Or, will it go to the left (more HI)? In this type of problem, the Kc value will be given. 5. 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. aA +bB cC + dD. This is because the activities of pure liquids and solids are equal to one, therefore the numerical value of equilibrium constant is the same with and without the values for pure solids and liquids. WebHow to calculate kc at a given temperature. 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. Example . So the root of 1.92 is rejected in favor of the 0.26 value and the three equilibrium concentrations can be calculated. The negative root is discarded. Since K c is being determined, check to see if the given equilibrium amounts are expressed in moles per liter ( molarity ). Given that [NOBr] = 0.18 M at equilibrium, select all the options that correctly describe the steps required to calculate Kc for the reaction., Kp = Kc (R T)n K p = K c ( R T) n. Kp: Pressure Constant. 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) Q=1 = There will be no change in spontaneity from standard conditions WebEquilibrium constants are used to define the ratio of concentrations at equilibrium for a reaction at a certain temperature. K increases as temperature increases. We can rearrange this equation in terms of moles (n) and then solve for its value. In this case, to use K p, everything must be a gas. 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 their knowledge, and build their careers. The concentration of each product raised to the power These will react according to the balanced equation: 2NOBr (g) 2NO (g) + Br2 (g). Here T = 25 + 273 = 298 K, and n = 2 1 = 1. Reactants are in the denominator. \[\ce{3 Fe_2O_3 (s) + H_2 (g) \rightleftharpoons 2 Fe_3O_4 (s) + H_2O (g)} \nonumber\]. WebTo use the equilibrium constant calculator, follow these steps: Step 1: Enter the reactants, products, and their concentrations in the input fields. Since we are not told anything about NH 3, we assume that initially, [NH 3] = 0. Kc is the by molar concentration. The concentrations of - do not appear in reaction quotient or equilibrium constant expressions. Why did usui kiss yukimura; Co + h ho + co. \[K = \dfrac{(a_{H_2O})}{(a_{H_2})}\nonumber\], \[K_p = \dfrac{(P_{H_2O})}{(P_{H_2})}\nonumber\], \[K_p = \dfrac{(0.003)}{(0.013)} = 0.23 \nonumber\]. Haiper, Hugo v0.103.0 powered Theme Beautiful Hugo adapted from Beautiful Jekyll Will it go to the right (more H2 and I2)? For this, you simply change grams/L to moles/L using the following: 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. A change in temperature typically causes a change in K, If the concentrations of a reactant or a product is changed in a system at constant temperature what will happen to the value of the equilibrium constant K for the system, The value of the equilibrium constant will remain the same, Using the data provided in the table calculate the equilibrium constant Kp at 25C for the reaction This tool calculates the Pressure Constant Kp of a chemical reaction from its Equilibrium Constant Kc. Why has my pension credit stopped; Use the gas constant that will give for partial pressure units of bar. and insert values in the equilibrium expression: 0.00652x2 + 0.002608x + 0.0002608 = x2 0.45x + 0.045. Example . Ab are the products and (a) (b) are the reagents. Step 2: List the initial conditions. [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 G = RT lnKeq. Kc is the by molar concentration. WebShare calculation and page on. 2 NO + 2 H 2 N 2 +2 H 2 O. is [N 2 ] [H 2 O] 2 [NO] 2 [H 2] 2. This problem has a slight trick in it. These will react according to the balanced equation: 2NOBr (g) 2NO (g) + Br2 (g). T: temperature in Kelvin. The partial pressure is independent of other gases that may be present in a mixture. 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 9) Let's plug back into the equilibrium constant expression to check: Example #10: At a particular temperature, Kc = 2.0 x 106 for the reaction: If 2.0 mol CO2 is initially placed into a 5.0 L vessel, calculate the equilibrium concentrations of all species. Step 2: List the initial conditions. T: temperature in Kelvin. What is the equilibrium constant at the same temperature if delta n is -2 mol gas . 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). Then, Kp and Kc of the equation is calculated as follows, k c = H I 2 H 2 I 2. Answer . In which direction will the reaction proceed, The reaction will proceed toward the products, An experiment involves the chemical system show below. It is associated with the substances being used up as the reaction goes to equilibrium. Answer . R: Ideal gas constant. All the equilibrium constants tell the relative amounts of products and reactants at equilibrium. Answer _____ Check your answer on Page 4 of Tutorial 10 - Solutions ***** The next type of problem involves calculating the value of Ksp given the solubility in grams per Litre. 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