Consider the following reaction: 2HI(g) <------> H2(g) + I2(g) If 2.77 moles of HI(g), 0.315 moles of H2, and 0.593 moles of I2 are at equilibrium in a 13.9 L container at 838 K, the value of the equilibrium constant, Kc, is ________.

Consider the following reaction: 2HI(g) <------> H2(g) + I2(g) If 2.77 moles of HI(g), 0.315 moles of H2, and 0.593 moles of I2 are at equilibrium in a 13.9 L container at 838 K, the value of the equilibrium constant, Kc, is ________.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.98PAE

See similar textbooks

Related questions

Q: Consider the following decomposition reaction: 2SO3(g) = 2SO2(g) + O2(g) When 12.0 mol of SO3 is…

Q: CO (g) + H2O (g) CO2 (g) + H2 (g) Kc = 0.0257 If a 2.00L vessel is charged with…

Q: Consider the following reaction where K. = 5.10×10-6 at 548 K. NHẠCI(s) =NH3(g) + HCI(g) A reaction…

A: The given equilibrium reaction is: NH4Cl(s) ⇌ NH3(g) + HCl(g) ; Kc = 5.10*10-6

Q: At a particular temperature, K = 2.6 x 10^-6 for the following balanced reaction: 2PCl3(g) + O2(g)…

A: Given : K = 2.6 x 10-6 Moles of PCl3 = 2.5 moles of O2 = 2.0 Volume = 3.0 L

Q: Phosgene is a potent chemical warfare agent that is now outlawed by international agreement. It…

A: Given, COCl2(g)⇌CO(g) + Cl2(g) Equilibrium constant (Kc) = 8.3x10-4 Equilibrium concentration of all…

Q: H2(g) + Clz(g) 2HCI(g) According to the reaction above, when 0.100 mol H2 and 0.100mol Cl were added…

A: Answer:- Firstly using the equilibrium equation, ICE table is written. Then using the expression and…

Q: Consider the following equilibrium system; 2HC1(g) + I2(s) 2HI(g) + Cl,(g) AH = - 254 kJ/mol Using…

Q: Calcium oxide and carbon dioxide react to form calcium carbonate, like this: CaO(s)+CO,(g)→CaCO;(s)…

A: Complete solution is given below in next step

Q: Consider the equilibrium system described by the chemical reaction below, which has a value of Kc…

A: The ICE table can be drawn as follows-

Q: Consider the equilibrium system described by the chemical reaction below, which has a value of Kc…

A: Given: The reaction is as follows, CaCrO4(s)⇌Ca2+(aq)+CrO42-(aq) At a particular temperature,…

Q: 1. At a particular temperature a flask at equilibrium contains [N2] of 1.40 x 10-4 M, [O2] of 1.25 x…

A: The chemical reaction is 2N2(g) + O2(g) ⇌2N2OGiven,N2=1.40×10-4 MO2=1.25×10-5MN2O=1.00×10-2M

Q: Consider the following system at equilibrium where AH° = -87.9 kJ, and K. 83.3, at 500 K: %3D PCI3…

A: The direction in which a reaction occurs, depends on several factors. The factors are temperature,…

Q: CH, (g) + H,0 (g) 3 H, (g) + CO (g) is brought to equilibrium at some steady temperature: when this…

Q: At a particular temperature, k=5.7x10-6 for the following balanced reaction: 2Cl2(g) + O2…

A: The balanced chemical reaction is as follows: The equilibrium constant for this reaction is given…

Q: A favorite reaction is calcite dissolution: CACO36) -→ Ca?+ + CO??- K = 10-83 Will the solid form or…

A: ANSWER : (a) Solid will be formed as we approach vent deep in the pacific Ocean. (b) Concentration…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: H2S and Oz react according to the equation below. Predict the equilibrium pressure of SO2. To do…

A: Given: Initial partial pressure of H2S = 2.00 Initial partial pressure of O2 = 5.00 Kp = 4.7×10-10…

Q: The equilibrium constant, Kc, is 4.20 × 10⁻⁶ at a temperature of 1100 K for the reaction: 2 H₂S₍₉₎…

A: Equillibrium constant is the ratio of concentaration of products to the concentration of reactants.

Q: Consider the following reaction where K, = 10.5 at 350 K. 2CH2CI2(g) CH4(9) + CCI4(g) A reaction…

Q: 2NO(g) + 2H₂(g) = N₂(g) + 2H₂O(g) Based on the equilibrium concentrations below, what is the value…

Q: Calculating an equilibrium constant from a heterogeneous equilibrium com... Calcium oxide and carbon…

A: Given, Mass of CaO = 10.8g. Mass of CO2 = 10.0g. Mass of CaCO3 = 80.1g. The given mass of components…

Q: 0/5 Calculating an equilibrium constant from a heterogeneous... Nitric acid and nitrogen monoxide…

Q: At a particular temperature a 2.00-L flask at equilibrium contains 5.10 × 10-4 moles of N2, 2.50 x…

A: The equilibrium reaction taking place is given as, => 2 N2 (g) + O2 (g) -------> 2 N2O (g)…

Q: The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600K. COCl2(g) CO(g) +…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

A: The reaction taking place will be 2 SO2 + O2 -------> 2 SO3

Q: Consider the following reaction where K. = 1.29×10-² at 600 K. COCI»(g) CO(g) + Cl2(g) A reaction…

Q: Question attached

A: Equilibrium constant Kc is defined as the product of concentration of products divided by the…

Q: .150 mol of COCl2(g) sealed in a volume of 10.0 L forms CO(g) and Cl2(g) at 360 °C. Use K =…

A: 0.150 mol of COCl2(g) sealed in a volume of 10.0 L forms CO(g) and Cl2(g) given K = 8.3×10–4 M…

Q: Part A Consider the reaction: SO2 Cl2 (g) = SO2 (g) + Cl2 (g) A reaction mixture is made containing…

Q: 1. A gaseous reaction mixture contains 0.30 atm SO2, 0.16 atm Cl2 and 0.50 atm SO2C)2 in a 2.0 L…

A: Given: PSO2=0.30 atmPCl2=0.16 atmPSO2Cl2=0.50 atm K= 0.011 To find: Whether the system is in…

Q: For the chemical equilibrium A + 2B ⇄ 2C, the value of the equilibrium constant, K, is 10. What is…

A: Given: Equilibrium constant (K) for the reaction A+ 2B ⇄ 2C is 10.

Q: Consider the equilibrium system described by the chemical reaction below, which has a value of Kc…

A: The given reaction is, CaCrO4(s) ⇌ Ca2+(aq) + CrO42-(aq)

Q: When 1.0 moles each of CO and Br2 were placed into a 1L container and allowed to reach equilibrium,…

Q: Part A Formamide, used in the manufacture of pharmaceuticals, dyes, and agricultural chemicals,…

Q: Consider the following reaction where Kc = 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) A reaction…

A: Given: Kc=5.10×10-6 at 548 KThe reaction taking place is : NH4Cl(s) → NH3(g)+HCl(g)Moles…

Q: In the following system: 3O2(g) + 2H2S(g) ⇌ 2H2O(g) + 2SO2(g) in a 500 mL container, the…

Q: Phosgene, COC12, is the chemical warfare gas commonly called mustard gas. It decomposes as 3)…

A: The equilibrium concentration is the ratio of equilibrium concentration of products to the…

Q: Consider the following system at equilibrium where AH° = -10.4 kJ, and K, = 55.6 , at 698 K: %3D H2…

Q: Consider the equilibrium, CO2(g) + H2(g) < ---- > CO(g) + H2O(g). Calculate the equilibrium…

A: Concentration of H2O = 0.46 M Concentration of H2 = 4.54 M Concentration of CO2 = 9.54 M Kc = 0.0049

Q: Consider the equilibrium system described by the chemical reaction below, which has a value of Kc…

A: Given data,Kc=7.1×10-4Given reaction,CaCrO4⇌Ca2++CrO42-

Q: Consider the following reaction where K. = 5.10×10-6 at 548 K. NH,CI(s): ENH3(g) + HCl(g) A reaction…

Q: Consider the following system at equilibrium where H° = 10.4 kJ, and Kc = 1.80×10-2, at 698 K.…

A: The given reaction: 2HI(g) ⇌ H2(g) + I2(g), ∆H° = 10.4 kJ As heat is consumed, this reaction is…

Q: The K. for CO (g) + 3 H2 (g) = CH4 (g) + H2O (g) is 9.17 * 10-2. If a 3.5 L vessel is set up with…

A: Normally for those chemical reactions , in which Kc value more than value of Qc , Reaction direction…

Q: A 100.-mL reaction vessel initially contains 2.60 × 10–2 mol of NO and 1.30 × 10–2 mol of H2. At…

Q: Consider the following system at equilibrium where AH° = -18.8 kJ, and K. = at 350 K:…

A: According to Le-Chatelier's principle, when a system is in equilibrium undergoes some change then it…

Q: The initial concentrations of four species involved in an equilibrium are: [Cl2] = 1.40 M, [HCl] =…

Q: A 100.-mL reaction vessel initially contains 2.60 × 10–2 mol of NO and 1.30 × 10–2 mol of H2. At…

A: The equilibrium constant, Keq for a reaction is given as :

Q: A 100.-mL reaction vessel initially contains 2.60 × 10–2 mol of NO and 1.30 × 10–2 mol of H2. At…

A: The given reaction is: Concentration is defined as moles / litre. Concentration of NO = 2.60×10-2…

Q: For the chemical SO2 + NO2= SO3 + NO The equilibrium constant at a certain temperature is 4.00. At…

A: Equilibrium constant only depends on temperature.if temperature same then equilibrium constant will…

Q: Consider the following system: 4 NH3(g) + 3 O2(g) -> 2 N2(g) + 6 H2O(l) AH = -1530.4 kJ (a) How…

A: Equilibrium is the state of the reaction where the rate of forward reaction is equal to the rate of…

Question

Consider the following reaction:

2HI(g) <------> H₂(g) + I₂(g)

If 2.77 moles of HI(g), 0.315 moles of H₂, and 0.593 moles of I₂ are at equilibrium in a 13.9 L container at 838 K, the value of the equilibrium constant, K_c, is ________.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]
1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L"' ofO2, what were the equilibrium concentrations of all species?
Consider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial concentrations are [O3]=1.0106M,[NO]=1.0105M,[NO2]=2.5104M, and [O2]=8.2103M , is the system at equilibrium? If not, in which direction does the reaction proceed? (b) If the temperature is increased, as on a very warm day, will the concentrations of the products increase or decrease? (HINT: You may have to calculate the enthalpy change for the reaction to find out if it is exothermic or endothermic.)
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
Red phosphorus is formed by heating white phosphorus. Calculate the temperature at which the two forms are at equilibrium, given white P: H f =0.00 kJ/mol; S =41.09 J/mol K red P: H f =17.6 kJ/mol; S =22.80 J/mol K
How is the strength of an acid related to the position of its ionization equilibrium? Write the equations for the dissociation (ionization) of HCI, HNO3, and HClO4in water. Since all these acids are strong acids, what does this indicate about the basicity of the Cl-, NO3, and ClO4ions? Are aqueous solutions of NaCl, NaNO3, or NaClO4basic?
For the reaction NH3(g)+H2S(g)NH4HS(s) K = 400. at 35.0C. If 2.00 moles each of NH3, H2S, and NH4HS are placed in a 5.00-L vessel, what mass of NH4HS will be present at equilibrium? What is the pressure of H2S at equilibrium?
A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.