If K for the following reaction is 5.4 x 1032 NO (g) + 02 (g) 2 NO2 (g)what is K for the reaction shown below?4 NO2 (g) 4 NO (g) + 2 02 (g)3.4 x 10 28O a.Ob,9x10141.9 x 10-14OC 27x1013rtO d 14.1.1x10e.29x1027

Answered: Image /qna-images/answer/7d78ad8b-33f9-4daf-9f71-e2fd847ecff2.jpg

If K for the following reaction is 5.4 x 10 13 2 NO (g) + 02 () ) 2 NO2 (g) what is K, for the reaction shown below? 4 NO2 (g) 4 NO (g) + 2 02 (g) O a. 3.4 x 10-28 O b.1.9 x 10-14 OC 2.7 x 1013 Od. 1.1 x 1014 d. e. 2.9 x 1027

If K for the following reaction is 5.4 x 10 13 2 NO (g) + 02 () ) 2 NO2 (g) what is K, for the reaction shown below? 4 NO2 (g) 4 NO (g) + 2 02 (g) O a. 3.4 x 10-28 O b.1.9 x 10-14 OC 2.7 x 1013 Od. 1.1 x 1014 d. e. 2.9 x 1027

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 12.89PAE

See similar textbooks

Related questions

Q: A chemist is studying the following reaction that has an equilibrium constant of 6.5 x 10²1/M *…

A: we need to calculate the reaction quotient from the given concentrations and after that compare the…

Q: At a given temperature, K. for the reaction 2 SO2(g) + O2(g) 2 SO;(g) is 2.4 × 10-3. What is the…

Q: 2NH3(g)↽−−⇀3H2(g)+N2(g)2NH3(g)↽−−⇀3H2(g)+N2(g) the equilibrium concentrations were found to be…

A: The reaction given be: 2NH3(g)↽−−⇀3H2(g)+N2(g) Given concentration at equilbrium [NH3]=0.250 M…

Q: The equilibrium constant expression for a gas reaction is K. = [H,O]°[SO2]² What balanced equation…

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

Q: At a given temperature, K for the reaction 2HCI (g) → H₂ (g) + Cl₂ (g) is 4.17x10-34. What is K for…

Q: 20) Consider the hypothetical reactions below. (1) A + 2B E → AB2 (2) A +B +→> AB K1 = 1x10 K2 =…

Q: Consider the following system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K.N2(g)…

A: The given reaction is:

Q: Consider the following reaction at 700 °C: 2N205(g) = 0z(g) + 4NO2(g) The equilibrium concentrations…

Q: Consider the following system at equilibrium where AH° = 18.8 k), and Kc = 9.52x10-2, at 350 K: CH4…

A: Le Chatelier's principle: This principle is used to predict the effect of a change in conditions on…

Q: Consider the following system at equilibrium where AH° = -16.1 kJ, and K.= 154 , at 298 K: 2 NO (g)…

A: According to Le-chatelier's principle when temperature of an exothermic reaction increases then the…

Q: Consider the reaction: kJ 2SO₂(g) + O₂(g)2SO3(g) AH=-198.2 mol How would the concentrations of SO₂,…

A: According to Le chatelier's principle" if an equilibrium is subjected to a change, equilibrium will…

Q: LU dCcess important values if needed for this question. Consider the following system at equilibrium…

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: The equilibrium constant expression for a gas reaction is…

A: When the rate of forward reaction is equal to the rate of backward reaction then the reaction is…

Q: The equilibrium constant is given for two of the reactions below. Determine the value of the missing…

A: Equilibrium of a reaction means rate of forward reaction is equal to the rate of backward reaction.…

Q: 4. What is the equilibrium constant for the reaction NO2(g) N204(g)? А. [NO2] [N204] В. [NO2]2…

A: The balanced reaction is – 2NO2 g⇔N2O4g

Q: = In the equilibrium reactions listed below, how many reactions show that Kp Rxn I: 2HI(g) →→→ H₂(g)…

A: Equilibrium constant(Kc) of a reaction is the ratio of the product of molar concentrations of…

Q: For the following reaction: H(g) + I(g) 2 HI(g) Keg = 50.5 If you mix together 2.0 x 10-2moles HI,…

Q: Consider the following system at equilibrium where AH° = 10.4 kJ, and K. = 1.80×10, at 698 K: 2HI(g)…

A: The reaction given is, => 2 HI (g) -------> H2 (g) + I2 (g) Given : ΔHo = 10.4 KJ and Kc =…

Q: 3. A solution with initial concentrations of 6.00 M Fe3+ and 10.0 M SCN is allowed to reach…

A: Option B is Correct Answer. [Fe3+] = 2.00 M ; [SCN-] = 6.00 M As the balanced reaction…

Q: Consider the following system at equilibrium where AH° = 108 kJ, and K. = 1.29×102, at 600 K:…

A: Given reaction is : COCl2 (g) <-----------> CO (g) + Cl2 (g) , ΔH0 = 108 KJ Equilibrium…

Q: At 1100 K, K, = 0.15 for the reaction 2502 (9) + O2(g) = 2SO3 (g) What is the value of K at this…

A: Since the relationship between Kp and Kc or K is given by => Kp = Kc X (RT)Δn = K X (RT)Δn…

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

A: Since the volume of system is decrease at constant temperature Hence according to ideal gas law we…

Q: Consider the following system at equilibrium where AH° = 87.9 kJ, and K. = 1.20×102, at 500 K: %3D…

A: From the thermodynamical data, it is cleared that the reaction is endothermic and the chemical…

Q: In the equilibrium reactions listed below, how many reactions show that Kp Kc. Rxn I: 2HI(g) →→→…

A: From the relation of Kp and Kc , one can determine whether Kp is greater than, smaller than, or…

Q: Consider the following system at equilibrium where AH° =-198 kJ, and K. = 34.5 , at 1.15×10° K: 2…

A: Based on the change in the enthalpy for the equilibrium reaction, the change in enthalpy given is…

Q: 2a

A: The effect of temperature on equilibrium according to LeChatlier's principle: When the forward…

Q: Consider the following reaction at equilibrium. What effect will removing H20 have on the system? 2…

A: Applying concept of equilibrium constant.

Q: At a certain temperature, the value of the equilibrium constant, K, for the reaction written below…

Q: 11. For the reaction! H2 + Cl2 = 2 HCI 5.512:1 If 5.0 mol of H2 and 3.0 mol of Cl2 are placed in a 2…

A: Given: moles of H2 = 5.0 mol moles of Cl2 = 3.0 mol Volume of flask = 2.0 L Equilibrium moles of H2…

Q: Based on your calculations, indicate whether each statement is True (T) or False (F): v1. Each…

A: Rate of a reaction is defined as the concentration change with time.

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

Q: The initial concentrations of four species involved in an equilibrium are: 2) [HCI] = 0.100 M, [O2]…

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: Co(g) + 2 H2(9) = CH;OH(g) K= 6.0 x 10-5 H2O(g) + C(s) = H2(9) + CO(g) K= 10. x 10-5 What is the…

A: Answer:- This question is answered by using the simple concept of calculation of value of…

Q: What MASS of carbon dioxide would be dissolved in an Olympic size swimming pool (2.5 x 106 L) that…

Q: Consider the following chemical equilibrium: 4 NH3(g) +3 0₂ (g) 2 N₂(g) + 6H₂O(g) Now write an…

A: The equilibrium constant of a reaction provides the relationship between the products and reactants…

Q: . Consider the equilibrium 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H₂O(g). Predict the effect on the…

Q: Consider the following system at equilibrium where AH° = -18.8 kJ, and K. = 10.5, at 350 K:…

Q: Consider the following system at equilibrium where AH° = -108 kJ, and Kc = 77.5, at 600 K: co (g) +…

A: Le Chatelier's principle: This principle is used to predict the effect of a change in conditions on…

Q: What is the equilibrium concentration of C? A(g) 2C(g) + B(g) + D(g) K = 6.0 x |3| 10-7 (In mol L-)…

Q: 20. What will happen to the equilibrium when more SO2 (g) is added to the following system? 2502(g)…

A: Le Châtelier’s principle explained the fact that whenever some changes are made in equilibrium…

Q: 4NH3(g) +302(g) =2N2(g) +6H20(g) The initit concentrations of NH3 and 02 are both 0.021 Mat a…

A: Given , Initial concentration of NH3 = 0.021 M O2 = 0.021 M [N2]eq = 0.00449 M Kc = ?

Q: the hypothetical reactions 1 and 2, K1 = 102 and K2 = 10–4. 1. A2(g) + B2(g) ↔…

A: Given- A2C+B2 (g)<->2AB(g)+1/2C2 Value of K=?

Q: Consider the following system at equilibrium where AH° = -111 kJ, and K. = 0.159, at 723 K. N2(g) +…

Q: Consider the following system at equilibrium where AH° = -18.8 kJ/mol, and K = 10.5, at 350 K:…

A: Since the reaction temperature has been decreased. And as per the le chatelier principle, the…

Q: 4 (a) Calculate the value of Kc for the reaction: PC15 (g) PC13 Cl2 (g) + (g) AH = Positive Given…

A: As per Le chateliers principle, when a system under equilibrium is subjected to any kind of stress,…

Q: 4. The balanced solubility equilibrium of CuS in aqueous ammonia is Cus(s) + 4 NH3 (aq) =…

A: The solubility equilibrium for CuS, solubility product and stability constants are given as follows,…

Question

If K for the following reaction is 5.4 x 103
2 NO (g) + 02 (g) 2 NO2 (g)
what is K for the reaction shown below?
4 NO2 (g) 4 NO (g) + 2 02 (g)
3.4 x 10 28
O a.
Ob,9x1014
1.9 x 10-14
OC 27x1013
rt
O d 14
.
1.1x10
e.29x1027

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider the reaction Fe3+(aq)+SCN(aq)FeSCN2+(aq) How will the equilibrium position shift if a. water is added, doubling the volume? b. AgNO3(aq) is added? (AgSCN is insoluble.) c. NaOH(aq) is added? [Fe(OH)3 is insoluble.] d. Fe(NO3)3(aq) is added?
Sulfuryl chloride, SO2Cl2 is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature, it decomposes to SO2 and Cl2. SO2Cl2(g) SO2(g) + Cl2(g)Kc = 0.045 at 375 C (a) A 10.0-L flask containing 6.70 g of SO2Cl2 is heated to 375 C. What is the concentration of each of the compounds in the system when equilibrium is achieved? What fraction of SO2Cl2 has dissociated? (b) What are the concentrations of SO2Cl2, SO2, and Cl2 at equilibrium in the 10.0-L flask at 375 C if you begin with a mixture of SO2Cl2 (6.70 g) and Cl2 (0.10 atm)? What fraction of SO2Cl2 has dissociated? (c) Compare the fractions of SO2Cl2 in parts (a) and (b). Do they agree with your expectations based on Le Chateliers principle?
Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
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?
Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the amount of ammonia at equilibrium be affected by 1. removing O2(g)? 2. adding N2(g)? 3. adding water? 4. expanding the container at constant pressure? 5. increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
The equilibrium constant for the reaction N2(g) + O2(g) 2 NO(g) is 1.7 103 at 2300 K. (a) What is K for the reaction when written as follows? N2(g) + O2(g) NO(g) (b) What is K for the following reaction? 2 NO(g) N2(g) + O2(g)
. Write the balanced chemical equation describing the dissolving of each of the following sparingly soluble salts in water. Write the expression for K for each process. a. AgIO3(s) c. Zn3(PO4)2(s) b. Sn(OH)2(s) d. BaF2(s)
The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?
Neither PbCl2 nor PbF2 is appreciably soluble in water. If solid PbCl2 and solid PbF2 are placed in equal amounts of water in separate beakers, in which beaker is the concentration of Pb2+ greater? Equilibrium constants for these solids dissolving in water are as follows: PbCl2(s) Pb2+(aq) + 2 Cl(aq)Kc = 1.7 105 PbF2(s) Pb2+(aq) + 2 F(aq)Kc = 3.7 108
Write the K_, expression for each of the following equilih ria for dissolution of the salt in water. Agl(s) *=* Ag+(aq) + I"(aq) Phl,(s)«=± Pb’+(aq) + 2 r(aq) Hg?L «=* Hg<+(aq) + 2 I_(aq) Cu(IO,)2 *=* Ctr+(aq) + 2 IO,-(aq)
Kc at 137 C is 4.42 for NO(g) + 12 Br2(g) NOBr(g) Calculate Kc at 137 C for 2NOBr(g) 2NO(g) + Br2(g)
Consider the system SO3(g)SO2(g)+12 O2(g)H=98.9kJ (a) Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by 1. adding oxygen gas. 2. compressing the system at constant temperature. 3. adding argon gas. 4. removing SO2(g). 5. decreasing the temperature. (b) Which of the above factors will increase the value of K? Which will decrease it?