how to find reaction quotient with partial pressure how to find reaction quotient with partial pressure

The concentration of component D is zero, and the partial pressure (or Solve Now. Insert these values into the formula and run through the calculations to find the partial pressures: This is the value for the equilibrium pressures of the products, and for the reactants, all you need to do is subtract this from the initial value Pi to find the result. The answer to the equation is 4. . Find the molar concentrations or partial pressures of each species involved. ), \[ Q=\dfrac{[\ce{C}]^x[\ce{D}]^y}{[\ce{A}]^m[\ce{B}]^n} \label{13.3.2}\], The reaction quotient is equal to the molar concentrations of the products of the chemical equation (multiplied together) over the reactants (also multiplied together), with each concentration raised to the power of the coefficient of that substance in the balanced chemical equation. Q > K: When Q > K, there are more products than reactants resulting in the reaction shifting left as more products become reactants. What is the value of the reaction quotient before any reaction occurs? We provide teachers with tools and data so they can help their students develop the skills, habits, and mindsets for success in school and beyond. It is a unitless number, although it relates the pressures. To find the reaction quotient Q, multiply the activities for the species of the products and divide by the activities of the reagents, raising each one of . Just make sure your values are all in the same units of atm or bar. . In this blog post, we will be discussing How to find reaction quotient with partial pressure. If a reaction vessel is filled with SO3 at a partial pressure of 0.10 atm and with O2 and SO2 each at a partial pressure of 0.20 atm, what can Using the reaction quotient to find equilibrium partial pressures How to divide using partial quotients - So 6 times 6 is 36. As a 501(c)(3) nonprofit organization, we would love your help!Donate or volunteer today! Find the molar concentrations or partial pressures of each species involved. If the same value of the reaction quotient is observed when the concentrations stop changing in both experiments, then we may be certain that the system has reached equilibrium. There are two types of K; Kc and Kp. The adolescent protagonists of the sequence, Enrique and Rosa, are Arturos son and , The payout that goes with the Nobel Prize is worth $1.2 million, and its often split two or three ways. But we will more often call it \(K_{eq}\). Thus for the process, \[I_{2(s)} \rightleftharpoons I_{2(g)} \nonumber\], all possible equilibrium states of the system lie on the horizontal red line and is independent of the quantity of solid present (as long as there is at least enough to supply the relative tiny quantity of vapor.). If instead our mixture consists only of the two products C and D, Q will be indeterminately large (10) and the only possible change will be in the reverse direction. Decide mathematic equation. If you're trying to calculate Qp, you would use the same structure as the equilibrium constant, (products)/(reactants), but instead of using their concentrations, you would use their partial pressures. Write the expression of the reaction quotient for the ionization of HOCN in water. He also shares personal stories and insights from his own journey as a scientist and researcher. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. How do you find the Q reaction in thermochemistry? For astonishing organic chemistry help: https://www.bootcamp.com/chemistryTo see my new Organic Chemistry textbook: https://tophat.com/marketplace/science-&-. Reaction Quotient Chemical Analysis Formulations Instrumental Analysis Pure Substances Sodium Hydroxide Test Test for Anions Test for Metal Ions Testing for Gases Testing for Ions Chemical Reactions Acid-Base Reactions Acid-Base Titration Bond Energy Calculations Decomposition Reaction Electrolysis of Aqueous Solutions Even explains (with a step by step totorial) how to solve the problem doesn't just simply give you the answer to you love that about it. The formula is: PT = P1 + P2 + P3 + PN Where PT is the. . A homogeneous equilibrium is one in which all of the reactants and products are present in a single solution (by definition, a homogeneous mixture). the numbers of each component in the reaction). The first, titled Arturo Xuncax, is set in an Indian village in Guatemala. The equation for Q, for a general reaction between chemicals A, B, C and D of the form: Is given by: So essentially it's the products multiplied together divided by the reactants multiplied together, each raised to a power equal to their stoichiometric constants (i.e. For example, the reaction quotient for the reversible reaction, \[\ce{2NO}_{2(g)} \rightleftharpoons \ce{N_2O}_{4(g)} \label{13.3.3}\], \[Q=\ce{\dfrac{[N_2O_4]}{[NO_2]^2}} \label{13.3.4}\], Example \(\PageIndex{1}\): Writing Reaction Quotient Expressions. anywhere where there is a heat transfer. It does not store any personal data. This can only occur if some of the SO3 is converted back into products. The reaction quotient aids in figuring out which direction a reaction is likely to proceed, given either the pressures or the . Only those points that fall on the red line correspond to equilibrium states of this system (those for which \(Q = K_c\)). The pressure given is the pressure there is and the value you put directly into the products/reactants equation. The data in Figure \(\PageIndex{2}\) illustrate this. each species involved. Solve math problem. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. The unit slopes of the paths and reflect the 1:1 stoichiometry of the gaseous products of the reaction. I can solve the math problem for you. 7.6 T OPIC: 7.6 P ROPERTIES OF THE E QUILIBRIUM C ONSTANT E NDURING U NDERSTANDING: TRA-7 A system at equilibrium depends on the relationships between concentrations, partial pressures of chemical species, and equilibrium constant K. L EARNING O BJECTIVE: TRA-7.D Represent a multistep process with an overall equilibrium expression, using the constituent K expressions for each individual reaction. Your approach using molarity would also be correct based on substituting partial pressures in the place of molarity values. Example \(\PageIndex{2}\): Evaluating a Reaction Quotient. To calculate Q: Write the expression for the reaction quotient. If G > 0, then K. In chemical thermodynamics, the reaction quotient (Qr or just Q) is a dimensionless quantity that provides a measurement of the relative amounts of products and reactants present in a reaction mixture for a reaction with well-defined overall stoichiometry, at a particular point in time. If the initial partial pressures are 0.80 atmospheres for carbon monoxide and 0.40 atmospheres for carbon dioxide, we can use the reaction quotient Q, to predict which direction that reaction will go to reach equilibrium. What is the value of the equilibrium constant for the reaction? For example, if we combine the two reactants A and B at concentrations of 1 mol L1 each, the value of Q will be 01=0. K is the numerical value of Q at the end of the reaction, when equilibrium is reached. 6 times 1 is 6, plus 3 is 9. 9 8 9 1 0 5 G = G + R . Since Q > K, the reaction is not at equilibrium, so a net change will occur in a direction that decreases Q. by following the same guidelines for deriving concentration-based expressions: \[Q_P=\dfrac{P_{\ce{C2H4}}P_{\ce{H2}}}{P_{\ce{C2H6}}} \label{13.3.20}\]. Before any product is formed, \(\mathrm{[NO_2]=\dfrac{0.10\:mol}{1.0\:L}}=0.10\:M\), and [N, At equilibrium, the value of the equilibrium constant is equal to the value of the reaction quotient. Why does equilibrium constant not change with pressure? A general equation for a reversible reaction may be written as follows: \[m\ce{A}+n\ce{B}+ \rightleftharpoons x\ce{C}+y\ce{D} \label{13.3.1}\], We can write the reaction quotient (\(Q\)) for this equation. Subsitute values into the expression and solve. Write the reaction quotient expression for the ionization of NH 3 in water. Using the ideal gas law we know that P= concentration (RT) and therefore Kp=Kc (RT)^n, when atm and molarity, the units for this problem . This example problem demonstrates how to find the equilibrium constant of a reaction from equilibrium concentrations of reactants and products . Write the expression to find the reaction quotient, Q. Q can be used to determine which direction a reaction Calculate G for this reaction at 298 K under the following conditions: PCH3OH=0.895atm and K is determined from the partial pressures. Answer (1 of 2): The short answer is that you use the concentration of species that are in aqueous solution, but the partial pressure of species in gas form. A system which is not necessarily at equilibrium has a partial pressure of carbon monoxide of 1.67 atm and a partial pressure of carbon dioxide of 0.335 . How do you calculate Q in Gibbs free energy? If K < Q, the reaction In some equilibrium problems, we first need to use the reaction quotient to predict the direction a reaction will proceed to reach equilibrium. A heterogeneous equilibrium is a system in which reactants and products are found in two or more phases. When the reaction reaches equilibrium, the value of the reaction quotient no longer changes because the concentrations no longer change. We can solve for Q either by using the partial pressures or the concentrations of the reactants and products because at a fixed temperature, the partial pressures of the reactants / products are proportional to their concentrations. K vs. Q This process is described by Le Chateliers principle: When a chemical system at equilibrium is disturbed, it returns to equilibrium by counteracting the disturbance. Do you need help with your math homework? For example, equilibria involving aqueous ions often exhibit equilibrium constants that vary quite significantly (are not constant) at high solution concentrations. Standard pressure is 1 atm. The concept of the reaction quotient, which is the focus of this short lesson, makes it easy to predict what will happen. Afew important aspects of using this approach to equilibrium: As a consequence of this last consideration, \(Q\) and \(K_{eq}\) expressions do not contain terms for solids or liquids (being numerically equal to 1, these terms have no effect on the expression's value). It may also be useful to think about different ways pressure can be changed. In Example \(\PageIndex{2}\), it was mentioned that the common practice is to omit units when evaluating reaction quotients and equilibrium constants. But, in relatively dilute systems the activity of each reaction species is very similar to its molar concentration or, as we will see below, its partial pressure. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Dividing by a bigger number will make Q smaller and youll find that after increasing the pressures Q. Kp is pressure and you just put the pressure values in the equation "Kp=products/reactants". The equilibrium partial pressure for P 4 and P 2 is 5.11 atm and 1.77 atm respectively.. c. K>Q, the reaction proceeds to the formation of product side in equilibrium.This will result in the net dissociation of P 4. There are actually multiple solutions to this. Advertisement cookies are used to provide visitors with relevant ads and marketing campaigns. As , EL NORTE is a melodrama divided into three acts. How to use our reaction quotient calculator? Re: Finding Q through Partial Pressure and Molarity. To calculate Q: Write the expression for the reaction quotient. The volume of the reaction can be changed. Determine the change in boiling point of a solution using boiling point elevation calculator. This relationship can be derived from the ideal gas equation, where M is the molar concentration of gas, \(\dfrac{n}{V}\). Reactions between solutes in liquid solutions belong to one type of homogeneous equilibria. These cookies help provide information on metrics the number of visitors, bounce rate, traffic source, etc. This cookie is set by GDPR Cookie Consent plugin. The equilibrium constant, KP, is still a constant, but its numeric value may differ from the equilibrium constant found for the same reaction by using concentrations. One reason that our program is so strong is that our . Concentration has the per mole (and you need to divide by the liters) because concentration by definition is "=n/v" (moles/volume). So in this case it would be set up as (0.5)^2/(0.5) which equals 0.5. However, the utility of Q and K is often found in comparing the two to one another in order to examine reaction spontaneity in either direction. Thus, our partial pressures equation still looks the same at this point: P total = (0.4 * 0.0821 * 310/2) nitrogen + (0.3 *0.0821 * 310/2) oxygen + (0.2 * 0.0821 * 310/2) carbon dioxide. A small value of \(K_{eq}\)much less than 1indicates that equilibrium is attained when only a small proportion of the reactants have been converted into products. For example K = \frac{[\mathrm{O_2(aq)}]}{[\mathrm{O. Register Alias and Password (Only available to students enrolled in Dr. Lavelles classes. Q is the net heat transferred into the systemthat is, Q is the sum of all heat transfer into and out of the system. Do math I can't do math equations. I believe you may be confused about how concentration has "per mole" and pressure does not. [B]): the ratio of the product of the concentrations of the reaction's products to the product of the concentrations of the reagents, each of them raised to the power of their relative stoichiometric coefficients. (Vapor pressure was described in the . The cookies is used to store the user consent for the cookies in the category "Necessary". Substitute the values in to the expression and solve for Q. If G Q, and the reaction must proceed to the right to reach equilibrium. D) It is an industrial synthesis of sodium chloride that was discovered by Karl Haber. A large value for \(K_{eq}\) indicates that equilibrium is attained only after the reactants have been largely converted into products. How to find reaction quotient with partial pressure Before any reaction occurs, we can calculate the value of Q for this reaction. Write the mathematical expression for the reaction quotient, Qc, for each of the following reactions: (a) CH4 ()+Cl2 ()CH3Cl ()+HCl () (b) N2 ()+O2 ()2NO () (c) 2SO2 ()+O2 ()2SO3 () a) Q = [CH3Cl] [HCl]/ [CH4] [Cl2] b) Q = [NO]2/ [N2] [O2] c) [SO3]2/ [SO2]2 [O2] 17. Q = heat energy (Joules, J) m = mass of a substance (kg) c = specific heat (units J/kgK) is a symbol meaning the change in T = change in temperature (Kelvins, K). Enthalpy (Delta H), on the other hand, is the state of the system, the total heat content. Find the molar concentrations or partial pressures of each species involved. Experts will give you an answer in real-time; Explain mathematic tasks; Determine math questions ), Re: Partial Pressure with reaction quotient, How to make a New Post (submit a question) and use Equation Editor (click for details), How to Subscribe to a Forum, Subscribe to a Topic, and Bookmark a Topic (click for details), Multimedia Attachments (click for details), Accuracy, Precision, Mole, Other Definitions, Bohr Frequency Condition, H-Atom , Atomic Spectroscopy, Heisenberg Indeterminacy (Uncertainty) Equation, Wave Functions and s-, p-, d-, f- Orbitals, Electron Configurations for Multi-Electron Atoms, Polarisability of Anions, The Polarizing Power of Cations, Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding), *Liquid Structure (Viscosity, Surface Tension, Liquid Crystals, Ionic Liquids), *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism), Coordination Compounds and their Biological Importance, Shape, Structure, Coordination Number, Ligands, *Molecular Orbital Theory Applied To Transition Metals, Properties & Structures of Inorganic & Organic Acids, Properties & Structures of Inorganic & Organic Bases, Acidity & Basicity Constants and The Conjugate Seesaw, Calculating pH or pOH for Strong & Weak Acids & Bases, Chem 14A Uploaded Files (Worksheets, etc. Find the molar concentrations or partial pressures of each species involved. The equilibrium constant for the oxidation of sulfur dioxide is Kp = 0.14 at 900 K. \[\ce{2 SO_2(g) + O_2(g) \rightleftharpoons 2 SO_3(g)} \nonumber\]. Expert Answer. Here's the reaction quotient equation for the reaction given by the equation above: If a reaction vessel is filled with SO3 at a partial pressure of 0.10 atm and with O2 and SO2 each at a partial pressure of 0.20 atm, what can you conclude about whether, and in which direction, any net change in composition will take place? the quantities of each species (molarities and/or pressures), all measured At equilibrium, \[K_{eq}=Q_c=\ce{\dfrac{[N2O4]}{[NO2]^2}}=\dfrac{0.042}{0.016^2}=1.6\times 10^2.\]. A system that is not at equilibrium will proceed in the direction that establishes equilibrium. states. Top Jennifer Liu 2A Posts: 6 Joined: Mon Jan 09, 2023 4:46 pm Re: Partial Pressure with reaction quotient You also have the option to opt-out of these cookies. Calculating the Equilibrium Constant Reaction Quotient: Meaning, Equation & Units. An equilibrium is established for the reaction 2 CO(g) + MoO(s) 2 CO(g) + Mo(s). You are correct that you solve for reaction quotients in the same way that you solve for the equilibrium constant. Q is a quantity that changes as a reaction system approaches equilibrium. Performance cookies are used to understand and analyze the key performance indexes of the website which helps in delivering a better user experience for the visitors. For example: N 2(g) +3H 2(g) 2N H 3(g) The reaction quotient is: Q = (P N H3)2 P N 2 (P H2)3 The expression for the reaction quotient, Q, looks like that used to The cookie is set by the GDPR Cookie Consent plugin and is used to store whether or not user has consented to the use of cookies. the concentrations at equilibrium are [SO2] = 0.90 M, [O2] = 0.35 M, and [SO3] = 1.1 M. What is the value of the equilibrium constant, Keq? For relatively dilute solutions, a substance's activity and its molar concentration are roughly equal. The amounts are in moles so a conversion is required. Find the molar concentrations or partial pressures of each species involved. Dividing by a bigger number will make Q smaller and you'll find that after increasing the pressures Q K. This is the side with fewer molecules. We use molar concentrations in the following examples, but we will see shortly that partial pressures of the gases may be used as well: \[\ce{C2H6}(g) \rightleftharpoons \ce{C2H4}(g)+\ce{H2}(g) \label{13.3.12a}\], \[K_{eq}=\ce{\dfrac{[C2H4][H2]}{[C2H6]}} \label{13.3.12b}\], \[\ce{3O2}(g) \rightleftharpoons \ce{2O3}(g) \label{13.3.13a}\], \[K_{eq}=\ce{\dfrac{[O3]^2}{[O2]^3}} \label{13.3.13b}\], \[\ce{N2}(g)+\ce{3H2}(g) \rightleftharpoons \ce{2NH3}(g) \label{13.3.14a}\], \[K_{eq}=\ce{\dfrac{[NH3]^2}{[N2][H2]^3}} \label{13.3.14b}\], \[\ce{C3H8}(g)+\ce{5O2}(g) \rightleftharpoons \ce{3CO2}(g)+\ce{4H2O}(g)\label{13.3.15a} \], \[K_{eq}=\ce{\dfrac{[CO2]^3[H2O]^4}{[C3H8][O2]^5}}\label{13.3.15b}\]. \(Q=\dfrac{[\ce C]^x[\ce D]^y}{[\ce A]^m[\ce B]^n}\hspace{20px}\textrm{where }m\ce A+n\ce Bx\ce C+y\ce D\), \(Q=\dfrac{(P_C)^x(P_D)^y}{(P_A)^m(P_B)^n}\hspace{20px}\textrm{where }m\ce A+n\ce Bx\ce C+y\ce D\). Will the reaction create more HI, or will some of the HI be consumed as the system moves toward its equilibrium state? Thus, the reaction quotient of the reaction is 0.800. b. Activities and activity coefficients Since K c is given, the amounts must be expressed as moles per liter ( molarity ). The denominator represents the partial pressures of the reactants, raised to the power of their coefficients, and then multiplied together. A general equation for a reversible reaction may be written as follows: (2.3.1) m A + n B + x C + y D We can write the reaction quotient ( Q) for this equation. arrow_forward Consider the reaction below: 2 SO(g) 2 SO(g) + O(g) A sealed reactor contains a mixture of SO(g), SO(g), and O(g) with partial pressures: 0.200 bar, 0.250 bar and 0.300 bar, respectively. Donate here: https://www.khanacademy.org/donate?utm_source=youtube\u0026utm_medium=descVolunteer here: https://www.khanacademy.org/contribute?utm_source=youtube\u0026utm_medium=desc forward, converting reactants into products. The cookie is used to store the user consent for the cookies in the category "Other. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. The line itself is a plot of [NO2] that we obtain by rearranging the equilibrium expression, \[[NO_2] = \sqrt{[N_2O_4]K_c} \nonumber\]. W is the net work done on the system. SO2Cl2(g) 24/7 help If you need help, we're here for you 24/7. The phases may be any combination of solid, liquid, or gas phases, and solutions. The only possible change is the conversion of some of these reactants into products. B) It is a process for the synthesis of elemental chlorine. CEEG 445: Environmental Engineering Chemistry (Fall 2021), { "2.01:_Equilibrium_Introduction" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.02:_Chemical_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.03:_Equilibrium_Constants_and_Reaction_Quotients" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.04:_Le_Chateliers_Principle" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Chemistry_Basics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Activity_and_Ionic_Strength" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Gas_Laws" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Acid-Base_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Solubility_and_Precipitation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Complexation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Redox_Chemistry_and_Electrochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Atmospheric_Chemistry_and_Air_Pollution" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Organic_Chemistry_Primer" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, 2.3: Equilibrium Constants and Reaction Quotients, [ "article:topic", "license:ccby", "showtoc:no", "Author tag:OpenStax", "authorname:openstax", "equilibrium constant", "heterogeneous equilibria", "homogeneous equilibria", "Kc", "Kp", "Law of Mass Action", "reaction quotient", "water gas shift reaction", "source[1]-chem-38268", "source[2]-chem-38268" ], https://eng.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Feng.libretexts.org%2FCourses%2FBucknell_University%2FCEEG_445%253A_Environmental_Engineering_Chemistry_(Fall_2020)%2F02%253A_Equilibrium%2F2.03%253A_Equilibrium_Constants_and_Reaction_Quotients, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), \[Q=\ce{\dfrac{[CO2][H2]}{[CO][H2O]}}=\dfrac{(0.0040)(0.0040)}{(0.0203)(0.0203)}=0.039.