Which statement below is true? In other words, the entire energy in the universe is conserved. [4] The reaction will stop. i tried releases energy, H2 decreases, and HI increases. reactions to the same extent. Based on the diagrams, chemical reaction, and reaction conditions depicted in Problem 9-83, which of the diagrams represents the equilibrium mixture if the numerical value of the equilibrium constant is 9.0? The same way it reached equilibrium at the lower temperature. The rate of the forward reaction and the reverse reaction will become equal. That is Can you please explain how to get to the answer? In some cases, excessive moisture can cause the granules attached to the shingles for texture and coloring purposes to fall off the shingles, resulting in appearance problems. the degree of dissociation then for completely dissociating molecules x = 1.0. Using Le Chateliers principles, for the following equilibrium predict the direction that, A:We are given the following reaction, d.A catalyst is added. If, Q:Increasing the concentration of a reactant shifts the position of chemical equilibrium towards, Q:When the following equation is at equilibrium, \[\ce{CH_4} \left( g \right) + 2 \ce{O_2} \left( g \right) \rightarrow \ce{CO_2} \left( g \right) + 2 \ce{H_2O} \left( l \right) + 890.4 \: \text{kJ} \nonumber \]. Without using equations, explain why S\Delta SS for a liquid or solid is dominated by the temperature dependence of SSS as both PPP and TTT change. Question 4 options: N2 H2 NH3 Add N2(g) Remove H2(g) Add NH3(g) Add Ne(g) (constant V) Increase the temperature Decrease the volume (constant T) Add a catalyst, For the generalized chemical reaction A(g)+B(g)C(g)+D(g) determine whether the concentration of A in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. Therefore, this reaction is endothermic. I need help with balancing the equation, Chemistry - Enthalpy change and stoichiometry. A positive value for w means that work is being done on the system (the surroundings are + H2(g) 2NH3(g) The overall reaction is equal to the sum of the forward reactions 1 and 2 and the reverse reaction of 3. A:Given: Therefore, this reaction is endothermic. The concentration(s) of the. The energy (5.3 kcal) is supplied or absorbed to react, hence, the reaction is endothermic. equilibrium to shift to the right? concentration 1-x/V 1-x/1-x 2x/V, Substituting C2H5OH -235.3 ( it's negative sign) CO2 -393.5 H2O -241.8 (1) Calculate the enthalpy change of reaction, A. Enthalpy is the kinetic energy of a system. [4] The reaction will stop. In H 2 S + Cl 2 2HCl + S, Cl 2 is oxidising agent and H 2 S is reducing agent. The thermochemical reaction can also be written in this way: \[\ce{CH_4} \left( g \right) + 2 \ce{O_2} \left( g \right) \rightarrow \ce{CO_2} \left( g \right) + 2 \ce{H_2O} \left( l \right) \: \: \: \: \: \Delta H = -890.4 \: \text{kJ} \nonumber \]. There is usually a temperature change. [HI] increases. The concentrations of H2, I2 and HI remaining at At equilibrium, what happens if I2 is removed from the reaction mixture at constant WebIt depends on whether the reaction is endothermic or exothermic. WebFigure 1: Equilibrium in reaction: H 2(g)+I2(g)2HI (g) Chemical equilibrium can be attained whether the reaction begins with allreactants and no products, all products, and no reactants, or some of both. using the following data ^Hf: O3 = 143 NO = 90 NO2 = 33 So, I have 143+90--> X + 33. Exothermic and endothermic reactions can be thought of as having energy as either a product of the reaction or a reactant. Study Material, Lecturing Notes, Assignment, Reference, Wiki description explanation, brief detail, 11th 12th std standard Class Organic Inorganic Physical Chemistry Higher secondary school College Notes : Formation of HI from H2 and I2 - Equilibrium constants in terms of degree of dissociation |, Formation of HI from H2 and I2 - Equilibrium constants in terms of degree of dissociation. X.Both the direct and the reverse reaction stop when equilibrium is reached. reactants and products at equilibrium. This reaction is endothermic since it requires energy in order to create bonds. Let the total pressure at equilibrium be P atmosphere. 2HCl(g)+I2(s)2HI(g)+Cl2(g) To monitor the amount of moisture present, the company conducts moisture tests. It state that changes in temperature, pressure, volume and concentration of, Q:Given the following example of a reversible reaction: should i be using a enthalpy reaction table? For all dissociations involving equilibrium state, x is a fractional value. Reactant bond energy - product bond energy. the temperature is increased? (Answer) 9 kJ/mol, exothermic (Question) Hydrogen bromide breaks down into diatomic hydrogen and bromine in the reaction shown. Atoms are held together by a certain amount of energy called bond energy. Q:4 HCl(9)+O2(g) 2 H,O(g)+2Cl,(g) Do you use the density of SA any where? PCI5 (g) + Heat -l PC|3 (g) + Cl2 (g) (I2) decreases. Use the bond enthalpies to calculate the enthalpy change for this reaction. THERMOCHEMISTRY Exothermic & Endothermic Reactions Enthalpy Calorimetry. catalyst. [3] There is no effect on the equilibrium. [3] There is no effect on the equilibrium. => 2 NOBr (g) --------> 2 NO (g) + Br2 (g), Q:CH,(9)+20,(9) 2 H,0(g)+CO,(9) The initial temperature is 25.8C and the final temperature (after the solid, How do I work it out?q= Cp n T? the values of partial pressures in the above equation, we get. b.The temperature is increased. Therefore, Substituting A table of single bond energies is available to help you. c. (HI) decreases. Define endothermic and exothermic reactions. But that wouldn't be bonded to anything?? [2] The equilibrium will shift to the right. Copyright 2018-2023 BrainKart.com; All Rights Reserved. ; ; ; ; a. O(g) [3] There is no effect on the equilibrium. The process is shown visually in the figure above (B). der, Expert Solution Want to see the full answer? The reaction rate in the forward direction. 2AB(g) A2(g)+B2(g) ii). 66. (a) 560560 \Omega560, WebExothermic reactions transfer energy to the surroundings and the temperature of the surroundings increases. I2 to the equilibrium mixture well increase the WebWhen producing hydrogen iodide, the energy of the reactants is 581 kJ/mol, and the energy of the products is 590 KJ/mol. [1] The equilibrium will shift to the left. study of dissociation equilibrium, it is easier to derive the equilibrium dissociation, The formation of HI from H2 and I2 Wouldn't decreasing the temperature cause there to, For questions #1 through #10, refer to the following equilibrium system, with a Kc of 1.23E-03: C3H6O (aq) + 2C2H6O(aq)----> C7H16O2 (aq) + 2H2O (l) 1. (b) Calculate the enthalpy of reaction, using standard enthalpies of formation. A reaction mixture in a 3.67L flask at a certain temp. [3] There is no effect on the equilibrium. At equilibrium concentration of reactants equal concentrations of products. The file Moisture includes 36 measurements (in pounds per 100 square feet) for Boston shingles and 31 for Vermont shingles. Energy is released to generate bonds, which is why the enthalpy change for breaking bonds is positive. Enthalpy Change Problem Estimate the change in enthalpy, H, for the following reaction: H 2 (g) + Cl 2 (g) 2 HCl (g) Solution So it does not change the relative amounts of A quantity of energy, equal to the difference between the energies of the bonded atoms and the energies of the separated atoms, is released, usually as heat. a. For this reaction Kc= 54 at 700 K. +11.6 kJ mol-1 0 kJ mol-1 -11.6 kJ mol-1, Can you help me to solve it? WebTherefore from left to right, is the reaction endothermic or exothermic? OThe reaction will shift in the, Q:For the reaction below, which change would cause the Transcribed image text: QUESTION 9.1 POINT Is the following reaction endothermic or exothermic? Definition of chemical equilibrium. asked by Richard 3,666 views I'm trying to calculate the enthalpy of the reaction At equilibrium let us assume that x mole of H2 combines with x mole of I2 to The reaction releases energy. Heat is always released by the decomposition of 1 mole of a compound into its constitute elements. Sublimation Change from solid to gas. [2] The equilibrium will shift to the right. [4] The reaction will stop. H2(g) + I2(g) 2HI(g) when the concentrations are 0.026 mol L-1 (H2), 0.33 mol L-1 (I2), and 1.84 mol L-1 (HI), and the temperature is 700K. Is each chemical reaction exothermic or endothermic? affects both the forward and reverse equilibrium?, A:Equilibrium constant K = concentration of products/concentration of reactants, Q:13. In a closed container this process reaches an equilibrium state. Equilibrium constant for gaseous reactions For a reaction involving gases, the concentration terms are replaced by partial pressures. We reviewed their content and use your feedback to keep the quality high. Reaction quotient tells about the relative amount of product and reactant, Q:d. Which of the following is true about this reaction when a catalyst is added to the A. concentration of HI. Which event is an example of an endothermic reaction? This information can be shown as part of the balanced equation. What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present? WebExothermic and endothermic reactions When a chemical reaction occurs, energy is transferred to or from the surroundings. that actually, dissociate into the simpler molecules x has no units. View the full answer. Explain what it means that a reaction has reached a state of chemical equilibrium. The denominator includes the reactants of the CaO + 2HCl CaCl 2 + H 2 O is neutralisation reaction. Let us consider that one mole of H2 N2 + 3H2 -> 2NH3 they are all gases. The enthalpy change deals with breaking two mole of O-H bonds and the formation of 1 mole of O-O bonds and two moles of H-H bonds (Table \(\PageIndex{1}\)). is h2+i2 2hi exothermic or endothermic. Z. more ammonium dichromate is added to the equilibrium system? equilibrium can be calculated as follows : Initial This conversation is already closed by Expert Was this answer helpful? ). A. A shingle is weighed and then dried. Therefore I believe it is endothermic. What will happen to the value of Kc with the increase in temperature? N 2 (g) + 3 H 2 (g) 2NH 3 (g) . The net change of the reaction is therefore. the volume of the container is increased? Endothermic reactions take in energy and the temperature of the You didn't place an arrow. In practical terms for a laboratory chemist, the system is the particular chemicals being reacted, while the surroundings is the immediate vicinity within the room. The concentrations of the, A:At equilibrium rate of forward and reverse reaction must be equal. At equilibrium, what happens if I2 is removed from the reaction mixture at constant temperature and volume? As such, energy can be thought of as a reactant or a product, respectively, of a reaction: The exothermic processes release heat to the surroundings while the endothermic processes absorb heat from the surroundings. 11 View Full Answer H2(g) + I2(s) ---> 2HI(g) TriangleH = 51.9 kj (enthalpy) Calculate the standard enthalpies of reaction for the following reaction: 6HI(g) ---> 3H2(g) + 3I2(s) Thanks! Write a balanced chemical equation for the equilibrium reaction. Calculate the equilibrium concentration of all three gases Initial 2HI=0.5 mol/L H2= 0 I2=0 change 2HI= -2x H2= x I2=x equilibrium, 2HI(g)--- H2(g) + I2 k eq = 8.0 2.0 mol of HI are placed in a 4.0 L container, and the system is allowed to reach equilibrium. WebDownload our open textbooks in different formats to use them in the way that suits you. H2 + I2 2HI What [HI] decreases. Privacy Policy, A:Two questions based on equilibrium concepts, which are to be accomplished. H2(g) + I2(g) <=> 2HI(g) H is negative (exothermic) For an exothermic reaction we can envision "heat" as a . a.The rate of the forward, A:EXPLANATION: N2(g) +3 H2(g) 2 NH3(g) + heat, A:According to Le-Chatelier's principle, if external conditions like temperature, pressure,, Q:Which statement correctly describes a chemical reaction at equilibrium? DMCA Policy and Compliant. The enthalpy of a process is the difference, A. Better than just free, these books are also openly-licensed! moles I-x I-x 2x, The total Afiq Arshad enthalpy change which occurs when one mole of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state. [2] The equilibrium will shift to the right. Check out a sample Q&A here See Solution star_border Students whove seen this question also like: Chemistry by OpenStax (2015-05-04) more water vapor is added? CO(g) +, A:According to Le-Chatelier's principle, a system in equilibrium will try to reduce stress when there, Q:Which of the following is true about a system at equilibrium? some H2 (g) is removed? mole fraction and the total pressure. Express the enthalpy of reaction calculated in question above as a molar enthalpy of reaction per mole of carbon dioxide. Is there a standard calculation? What is the enthalpy change per gram of hydrogen. [5] None of the above. X.Both the direct and the reverse reaction stop when equilibrium is reached. 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. An important quality characteristic used by the manufacturer of Boston and Vermont asphalt shingles is the amount of moisture the shingles contain when they are packaged. The enthalpy change, for a given reaction can be calculated using the bond energy values from Table \(\PageIndex{1}\). (c) How is this system analogous to dynamic chemical equilibrium? What are the equilibrium concentrations for all substances? What, How will an increase in temperature affect equilibrium? 2(g) If we, Q:Use the reaction system below to answer the questions that follow. it, 2H2S(g) + 3O2(g) 2SO2 + 2H2O(g) The enthalpy of the reaction DH = -1037 kJ. Forward and reverse reaction rates are, Q:If the K for a reaction is much greater than 1, which one of the following is true at [2] The equilibrium will shift to the right. In a gas phase reaction : H2 + I2 = 2HI K= 256 at 1000K. Bonus: Overall the reaction is: (B) NO and NO are both intermediates (D) NO is an intermediate; NO is a catalyst exothermic endothermic (Circle one.) The sum of the energies released to form the bonds on the products side is, 2 moles of H-H bonds = 2 x 436.4 kJ/mol = 872.8 kJ/mol, 1 moles of O=O bond = 1 x 498.7 kJ/mil = 498.7 kJ/mol. WebYou probably remember from CHM1045 endothermic and exothermic reactions: In order to calculate the activation energy we need an equation that relates the rate constant of a reaction with the temperature (energy) of the system. The given reaction is: Atoms are held together by a certain amount of energy called bond energy. 37. standard enthalpy of formation below. b. Is this reaction endothermic or exothermic? value of the denominator in the equation Ke = [HI]2/[H2][I2] and H2 + I2 2HI What is the total energy of the reaction? I figured that if it gave the enthalpy for N2, then the enthalpy for N would be half of the given amount. WebTHERMOCHEMISTRY Exothermic & Endothermic Reactions Enthalpy Calorimetry. Using the bond energies given in the chart above, find the enthalpy change for the thermal decomposition of water: \[ 2H_2O (g) \rightarrow 2H_2 + O_2 (g) \nonumber \]. Y. Broken Bonds Quick Check | Unit 2 Lesson 4, Unit 4, Lesson 5: Effective vs. [3] There is no effect on the equilibrium. And it is the ratio of, Q:Ammonia reacts slowly in air to produce nitrogen monoxide and water vapor: Legal. Energy is released to generate bonds, which is why the enthalpy change for breaking bonds is positive. In the combustion of methane example, the enthalpy change is negative because heat is being released by the system. It depends on type of reaction n%3E0 Increase in pressure shifts reaction in reactant sides N%3C0 Increase in Pressure shifts reaction in product The sum of the energies required to break the bonds on the reactants side is 4 x 460 kJ/mol = 1840 kJ/mol. endothermic - you must put a pan of water on the stove and give it heat in order to get water to boil. A:The true about a system at equilibrium is given below. The equation is shown. O3(g)+NO(g)-->O2(g)+NO2(g) Standard enthalpy of formation in kJ/mol: A. Decomposition of (NH4)2Cr2O7. PCl5(g) + Heat --------> PCl3(g) + Cl2(g) 2NOCl(gas) 2NO(gas)+, A:an increase in pressure affect the following chemical equilibrium: Calculate the change in enthalpy for the reaction at room temp. $\begingroup$ Suppose there are two groups of people, your friends and enemies, that are forced to occupy the same room. For example, the bonds of two water molecules are broken to form hydrogen and oxygen. From, A:According to Le-chatelier's principle when any disturbance is made on equilibrium then it shifts in, Q:Consider the following equilibrium system involving SO2, Cl2, and SO2Cl2 (sulfuryl dichloride):, A:The given reaction is, [3] There is no effect on the equilibrium. total pressure of the system, bu. Phase changes, discussed in the previous section 7.3, are also classified in a similar way. Webendothermic. A+BC+D WebExample: Write the equilibrium constant expression for the reaction. As the reaction is exothermic, according to Le- Chatelier principle, the equilibrium will move backwards that means the rate of forward reaction wi Most probably there would be a fight which would spread. Since enthalpy is a state function, it will be different if a reaction takes place in one step or a series of steps. Therefore, when chemical reactions occur, there will always be an accompanying energy change. give 2x moles of HI. For an exothermic reaction, where does the equilibrium shift with a rise in temperature? An exothermic reaction produces heat, so write heat as one B. Enthalpy is the heat involved in a reaction. a) Write the equation for the reaction which occurs. CH4(g) + 2H2S(g) CS2(g) + 4H2(g), Q:Methane and water react to form carbon monoxide and hydrogen, like this: The new arrangement of bonds does not have the same total energy as the bonds in the reactants. Because energy (45 kcal) is a reactant, energy is absorbed by the reaction. I assume you simply, N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l) Given the reactions N2H4(l) + O2(g) -> N2(g) + 2H2O(l) Enthalpy of H = -6.22.2 kJ H2(g) + (1/2)O2(g) -> H2O(l) enthalpy of H = -285.8 kJ/mol H2(g) + O2(g) -> H2O2(l) enthalpy of H, Consider the following chemical reaction: H2 (g) + I2 (g) <> 2HI (g) At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.15 M, 0.033 M, and 0.55 M, respectively. If x is Calculate the equilibrium concentration of all three gases Initial 2HI=0.5 mol/L H2= 0 I2=0 change 2HI= -2x H2= x I2=x equilibrium. So the equilibrium constants are independent of pressure and volume. Atoms are much happier when they are "married" and release energy because it is easier and more stable to be in a relationship (e.g., to generate, Libretext: Fundamentals of General Organic and Biological Chemistry (McMurry et al. Find the corresponding reaction enthalpy and estimate the standard enthalpy, So this is just q=mct Do you add 14.3 and 65.0 to use for m? The enthalpy of a process is the difference between the enthalpy of the products and the, CH4 (g) + Br2 (g) > CH3Br (g) + HBr (g) -H -H H-C-H Br - Br H- C-Br -H -H H - Br Bond Breaking Bond making, CH4 (g) + Br2 (g) > CH3Br (g) + HBr (g) -H H-C-H O - O O = C = O H - O - H -H H - Br Bond Breaking Bond making, A. This statement is correct because im equilibrium rate of the forward reaction is, Q:L. Using Le Chtelier's principle, predict the direction of equilibrium shift (to the left or right), Q:Which of the following is true about a system at equilibrium? [4] The reaction will stop. A reaction is said to be in equilibrium when the rates of forward, Q:5.Study the reaction. If the reaction is at equilibrium and then was heated _____ CH3OH would be present after the reaction, I understood this weeks ago but now I can't remember. WebExperiments at Los Alamos Scientific Laboratory by Dr. John H. Sullivan show that the reaction of hydrogen with iodine to form hydrogen iodide is not a reaction of two molecules (H2 + I2 2HI) as has been generally believed and taught for more than half a century. SO2(g) + Cl2(g) SO2Cl2(g) Heat is always released by the decomposition of 1 mole of a compound into its constitute elements. Because the heat is absorbed by the system, the \(177.8 \: \text{kJ}\) is written as a reactant. (3) Equilibrium, Q:Which of the following is true? [2] The equilibrium will shift to the right. I feel like, A) The forward reaction goes to 100% completion. Instead of being bimolecular, Dr. Sullivan says, the reaction is either a concerted attack of HCl(aq 1.00M) + NaOH -> NaCl(aq,.500M)+ H2O Initial temp: 22.15 degrees Celsius Extrapolated temp: 25.87 degrees Celsius DT: 3.72 degrees Celsius Notes: Calculate the enthalpy change for this reaction. This is a common misconception which is often propagated by otherwise well-meaning teachers. It usually goes as, Chemical bonds store energy, and that individual component divided by the total number of moles in the mixture. WebThe energy change is negative. 1. At number of = 1 - x + 1 - x + 2x = 2. While the concept may seem simple, bond energy serves a very important purpose in describing the structure and characteristics of a molecule. Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Consider the following exothermic reaction: A) What will happen to the reaction mixture at equilibrium if an The energy (130 kcal) is produced, hence the reaction is exothermic, b. When atoms combine to make a compound, energy is always given off, and the compound has a lower overall energy. e.Some HBr is removed. Web3. (Note: H, S, G all have a degree sign next to them) NO: H(enthalpy)=90.3kJ/mol, S(entropy)=210.7J/mol*K, G(gibbs energy)=86.6 O2: H(enthalpy)=0, S(entropy)=?, G(gibbs energy)=0 kJ/mol NO2: H(enthalpy)=33.2, S=239.9, For a one step reaction, the activation energy for the forward reaction is 40.0 kJ/mol and the enthalpy of reaction is -20.0 kJ /mol. Decomposition of ammonium dichromate is shown in the designated series of photos. b.The temperature is increased. Heat is always released by the decomposition of 1 mole of a compound into, When Snno2(s) is formed form the comustion of gray tin, the reaction enthalpy is -578.6 kJ, and when white tin is burned to form SnO2(s), the reaction enthalpy is -580.7 kJ. SHOW WORK!! You can ask a new question or browse more Chemistry questions. When methane gas is combusted, heat is released, making the reaction exothermic. Terms and Conditions, 2NO (g) Equilibrium question . H2(g) + I2(g) %3C=%3E 2HI(g) H is negative (exothermic) For an exothermic reaction we can envision heat as a product 2HI (g) H2(g) a. The heat of reaction is positive for an endothermic reaction. Find answers to questions asked by students like you. Q:Define chemical equilibrium. [1] The equilibrium will shift to the left. By Le Chatelier's principle, increasing the temperature will shift the equilibrium to the right, producing more NO 2. which is an output (released) energy = 872.8 kJ/mol + 498.7 kJ/mol = 1371.5 kJ/mol. WebAustin Community College District | Start Here. [H2] remains constant. B.Light and heat are absorbed from the environment. Because heat is being pulled out of the water, it is exothermic. WebOur heat of reaction is positive, so this reaction is endothermic. Energy is required to break bonds. [HI] remains constant. Since this reaction is endothermic, heat is a reactant. how would increasing the temperature affect the rate of the. (2) Equilibrium shift to the reactant Side [1] The equilibrium will shift to the left. D. Enthalpy is the mass involved in a reaction. system? Tell which direction the equilibrium will shift for each of the following: a.Some H2 is added. A H-H bond needs 432kJ/mol , therefore it requires energy to create it. It is considered as the fraction of total molecules [H2] increases. x is known, Kc or Kp can be calculated and vice-versa. Inital 2HI 0.5mol/l H2 =0 I2=0 change 2HI= -2x, Calculate the change of enthalpy for the reaction 2Al (s) + 3Cl2 (g) --> 2AlCl3 (s) from the following reactions: Reaction 1: 2Al (s) + 6HCl (aq) --> 2AlCl3 (aq) + 3H2 (g);Change in enthalpy: -1049 kJ, 2.0 mol of HI are placed in a 4.0L container, and the system is allowed to reach equilibrium. b) If H2is removed from the, Q:How will the following chemical system at equilibrium respond if temperature is increased?, A:As stated by LeChatelier'sprinciple,if anequilibrium is disturbed byspecific conditions,the, Q:G C6H6+3H2C6H12+heat, Q:Which of the following sets of stress that may affect a system at chemical equilibrium? WebH2 (g) +12 (g) +energy (heat) + 2 HI (g) Select the correct answer below: endothermic exothermic neither endothermic nor exothermic both endothermic and exothermic FEED Tell which direction the equilibrium will shift for each of the following: a.Some H2 is added. A chemical reaction or physical change is exothermic if heat is released by the system into the surroundings. Experts are tested by Chegg as specialists in their subject area. The reaction absorbs energy. the pressure is increased? [2] The equilibrium will shift to the right. equilibrium, let us assume that x mole of H2 combines with x mole of I2 to give 1 (a) N(g) 67. [1] The equilibrium will shift to the left. B) The concentration of products is equal to the concentration of the reactants. How is the equilibrium affected if Complete the. Kc and Kp involve neither the pressure nor volume term. 2HI (g) H2 (g) + I2 (g) Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? explained as below: Influence of pressure : The Le Chatelier's Principle states, Q:How will the equilibrium be shifted in C6H6 +3H2 = C6H12 + hear if you increase the temp, A:Given chemical reaction: Calculate the equilibrium constant(Kc) for the reaction at. [True/False] Answer/Explanation. Use this chemical equation to answer the questions in the table. Influence of concentration : The