Two reactions and their equilibrium constants are given.A + 2 B= 2CK1 = 2.972C DK2 = 0.170Calculate the value of the equilibrium constant for the reaction D A + 2 B.K =

Answered: Image /qna-images/answer/3597d4d8-af1f-4f69-8613-722838bba458.jpg

Answered: Two reactions and their equilibrium…

Two reactions and their equilibrium constants are given. A + 2B 2C K1 = 2.97 2 C D K, = 0.170 Calculate the value of the equilibrium constant for the reaction D A + 2B. K =

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter13: Fundamental Equilibrium Concepts

Section: Chapter Questions

Problem 6E: Explain why there may be an infinite number of values for the reaction quotient of a reaction at a...

See similar textbooks

Related questions

Q: Consider the reaction that occurs during the Haber process: N2(8) + 3 H2(g) –→ 2 NH,(8) The…

A: Given: The reaction is as follows: N2(g)+3H2(g)→2NH3(g) Equilibrium constant(K1)=3.9×105 At 3000C…

Q: Consider the reactions and their respective equilibrium constants: NO(8) + įBr2(8) = NOB1(g) Kp =…

A: Consider the target equation as; N2 g + O2 g + Br2 g ⇌ 2 NOBr g Consider the given reactions…

Q: Consider the reactions and their respective equilibrium constants: NO(g) +Br(g) NOBI(g) Kp = 5.3 2…

A: Equilibrium constant possessing specified reactants-products gets changed on reversing that…

Q: Write the equilibrium constant expression, K, for the following reaction taking place in dilute…

A: The solution is given below -

Q: Consider the reaction: P(s) + 3/2 Cl2(g)PCl3(g) Write the equilibrium constant for this reaction in…

A: A + B ⇔C + D. This is a reversible reaction where reactants give raise to products and products also…

Q: 2NO2(g) = N2O4(8) 25O2(g) + 02(g) = 2S03(g) 2SO2 H2(g) + Cl2(g) = 2HCI3)

Q: For the liquid-phase reaction A + 2B ⇄ 2C + D , it was found that when 2 mol A, 4 mol B and 2 mol C…

A: Since initially we have 0 moles of D Hence moles of D formed = moles of A reacted as from the…

Q: Express the equilibrium constant for the following reaction. 2 P4O10(s) ⇌ 2 P4(s) + 10 O2(g) A)…

Q: Calculate the value of the equilibrium constant K, for the reaction 2D = A+ 2B from the following…

A: please find the attachment.

Q: Balance each of the following examples of heterogeneousequilibria and write its reaction quotient,…

A: Balanced chemical equation of a reaction is written according to law of conservation of mass.…

Q: Write the equilibrium-constant, Kp, expression for the reaction A(g) + 4 B(1) = 3 C(g) + D(g) Answer…

Q: The equilibrium constant K, for the reaction HCN(aq) =H*(aq) + CN (aq) is 4.9 x 10-10 at 25 °C.…

A: The equilibrium concentration can be calculated as follows

Q: For the reaction: NO(g) + 1/20,(g) NO2(g) at 750 C, the equilibrium constant, K, equals а) 1.0 b) К,…

Q: Write the equilibrium constant expressions (Ke and Kp) for the following reactions: a. 4NH3 (g) +…

A: Introduction : We have to calculate Kp and Kc . As per company norms we cannot answer more than 3…

Q: The equilibrium constant for the reaction Na2(g) → 2Na(g) is 2.47 at 1000. K. Calculate the value of…

A: given chemical equilibrium Na2 ⇋2Na we are required to find the value of Gibbs free energy if…

Q: An equilibrium mixture from the following reaction was found to contain 1.20 mol dm-3 of A, 1.00 mol…

Q: equilibrium constant

Q: Write the equilibrium constant expressions for Kc and Kp, if applicable, for the following…

A: For a reversible reaction, the value of the reaction quotient at equilibrium is known as the…

Q: The equilibrium constant for the reaction Na,(g) – 2Na(g) is 2.47 at 1000. K. Calculate the value of…

Q: Given the two reactions shown with their equilibrium constants at a particular temperature: 2…

Q: Calculate the value of the equilibrium constant, K, for the reaction Q(g) + X(g) 2 M(g) + N(g) given…

Q: The conventional equilibrium constant expression (Kc) for the system as described by the below…

A: We have to predict the Equilibrium constant expression for the given reaction .

Q: Two reactions and their equilibrium constants are given. A + 2B 2C K1 = 2.75 2 C D K2 = 0.218…

Q: Consider the reaction: P(s) + 5/2 Cl2(g)PCl5(g) Write the equilibrium constant for this reaction in…

A: We have to write the equilibrium constant for this reaction in terms of the equilibrium constants,…

Q: Two reactions and their equilibrium constants are given. A + 2 B 20 K1 = 2.05 2C D K2 = 0.158…

Q: The equilibrium constant, K, for the synthesis of ammonia 6.8 x 105 at 298 K. Predict the value at…

A: Given , Reaction : N2+3H2⇋2NH3 Equilibrium constant at temperature , T1= 298 K , K1= 6.8×105 {…

Q: 2NO2(g) = N204(g) 2SO2(g) + 02(g) = 2SO3(g)

Q: For the following combustion reactions, predict whether compression will favour the formation of…

Q: If, at a given temperature, the equilibrium constant for the reaction H2(g) + Cl2(g) 2HCl(g) is Kp,…

A: Given reaction and information, The equilibrium constant for the reaction H2(g) + Cl2(g)…

Q: Consider the following reactions and their respective equilibrium constants: NO (g) + ½ Brz (g) NOBI…

A: Rearranging this equation 2 and equation 3, N2O4 (g) →2NO (g)+O2…

Q: The equilibrium constant (K1) for the reaction CO2 (g) 2 CO(g) +1/2 02(8) is 6.66 x 10-12 at 1000 K.…

A: CO2(g) -> CO(g) + 1/2O2 K1= 6.66 × 10^-12

Q: Write the mathematical expression for the reaction quotient, Qc, for each of the following…

A: The reaction quotient (Q) measures the relative amounts of products and reactants present during a…

Q: Consider an initial pressure of I2(g) of 0.100 atm in a 500 mL flask at 1000 K. With an equilibrium…

A: The initial pressure of I2 = 0.1atm Volume of flask = 500ml Kp = 3.76×10-3 We have to find the total…

Q: Two reactions and their equilibrium constants are given. A + 2B= 2C Kj = 2.21 2c D K2 = 0.104…

A: Two reactions at equilibrium are as follows: The equilibrium constant expression for these…

Q: Two reactions and their equilibrium constants are given. A + 2B 20 K1 = 2.39 2 C D K2 = 0.150…

Q: Consider the following reactions and their associated equilibrium constants: K1 A+ 2B S C C= D+E K2…

A: Given A + 2B ⇌C ( K1) C ⇌D + E (K2) A + 2B ⇌ D +E Kc = ?

Q: The equilibrium constant (K₁) for the reaction K₂ = CO₂(g) CO(g) + 1/2O₂(g) is 6.66 x 10-¹2 at 1000…

Q: The equilibrium constant for the reaction N2(g) + O2(g) ⇋ 2 NO(g) is 1.69 × 10−3 at 2300 K. A…

A: Equilibrium constant of a reaction is calculated by taking ratio of multiplication of concentration…

Q: Two reactions and their equilibrium constants are given. A + 2 B 2c Kj = 2.67 2 C D K2 = 0.270…

Q: The equilibrium constant for the reaction Na2(g) → 2Na(g) is 2.47 at 1000. K. Calculate the value of…

A: A question based on chemical thermodynamics that is to be accomplished.

Q: The equilibrium constant for the generic reaction : A(g) + 3B(g) ⇄ 2C(g) is Keq=1.8x104…

A: Given A(g) + 3B(g) ⇌ 2C Equilibrium Constant ( K1 ) = 1.8 × 104 4C ⇌ 2A(g) +…

Q: Consider the reaction: C(s) + 02(g)CO,(g) Write the equilibrium constant for this reaction in terms…

A: The given equilibrium reactions are: C(s)+O2g⇌CO2g; K ......(1)C(s)+12O2g⇌COg; Ka…

Q: Consider the following equilibria at a given temperature: K= 6.45 x 10, 1½N2(g) + ½0>(g) = NO(g)…

A: Equilibrium constant is defined as products concentrations divided by reactant concentrations to the…

Q: The equilibrium constant Kc for C + CO2 <=> 2CO is 1.9 at 1000 K and 0.133 at 298K. Is the…

A: It is given that Kc at 1000 K is 1.9 for the given reaction and the Kc at 298 K is 0.133, and the…

Q: The equilibrium constant, Kp. for the following reaction is 0.444 at 452 K: (CHy),CHOH(9) R…

A: We can write kp for a given reaction as A ----> B + C Kp= PB×PC/ PA And using this equation we…

Q: 2. The equilibrium constant for the reaction: C02(g) CO(g) + 1/2 0,(g) is 6.66 × 1012 at 1000 K.…

A: The equilibrium constant for the reverse reaction is the reciprocal of the Keq of the forward…

Q: For the reaction of 2NO2 (g) ↔ 2NO (g) + O2 (g), as Kc = 1.8 × 10-6 at 184 ° C, What is the…

Q: Balance each of the following examples of heterogeneousequilibria and write its reaction quotient,…

A: To find: Balancing the given reaction Determination of reaction quotient

Question

Two reactions and their equilibrium constants are given.
A + 2 B= 2C
K1 = 2.97
2C D
K2 = 0.170
Calculate the value of the equilibrium constant for the reaction D A + 2 B.
K =

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

Final Answer

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at this temperature in units of kJ/mol.
Write the mathematical expression for the reaction quotient, QC, for each of the following reactions (a) N2(g)+3H2(g)2NH3(g) (b) 4NH3(g)+5O2(g)4NO(g)+6H2O(g) (C) N2O2(g)2NO2(g) (d) CO2(g)+H2CO(g)+H2O(g) (e) NH4CI(s)NH3(g)+HCI(g) (f) 2Pb( NO3)2(s)2PbO(s)+4NO2(g)+O2(g) (g) 2H2(g)+O2(g)2H2O(g) (h) S8(g)8S(g)
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
What is the approximate value of the equilibrium constant KP for the change C2H5OC2H5(l)C2H5OC2H5(g) at 25 C. {Vapor pressure was described in the previous Chapter on liquids and solids; refer back to this chapter to find the relevant information needed to solve this problem.)
The equilibrium constant for the dissociation of iodine molecules to iodine atoms I2(g) 2 I(g) is 3.76 103 at 1000 K. Suppose 0.105 mol of I2 is placed in a 12.3-L flask at 1000 K. What are the concentrations of I2 and I when the system comes to equilibrium?
Explain why there may be an infinite number of values for the reaction quotient of a reaction at a given temperature but theme can he only one value for the equilibrium constant at that temperature.
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
Carbon dioxide decomposes into CO and O2 at elevated temperatures. What is the equilibrium partial pressure of oxygen in a sample at 1000 C for which the initial pressure of CO2 was 1.15 atm?
Consider the following equilibria involving SO2(g) and their corresponding equilibrium constants. SO2(g) + 12 O2(g) SO3(g) K1 2SO3(g) 2SO2(g) + O2(g) K2 Which of the following expressions relates K1 to K2? (a) K2=K12 (b) K22=K1 (c) K2 = K1 (d) K2 = 1/K1 (e) K2=1/K12
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
Methanol can be synthesized by means of the equilibriumreaction CO(g)+2H2(g)CH3OH(g) for which the equilibrium constant at 225°C is 6.08103. Assume that the ratio of the pressures of CO(g) and H2(g) is 1:2. What values should they have if the partial pressureof methanol is to be 0.500 atm?
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (a) 2NH3(g)N2(g)+3H2(g) Kc=17;[NH3]=0.50M,[N2]=0.15M,[H2]=0.12M (b) 2NH3(g)N2(g)+3H2(g) Kp=6.8104 initial pressures NH3=2.00atm,N2=10.00atm,H2=10.00atm (c) 2SO3(g)2SO2(g)+O2(g) Kc=0.230;[SO3]=2.00M,[SO2]=2.00M,[O2]=2.00M (d) 2SO3(g)2SO2(g)+O2(g) Kp=16.5 initial pressures SO2=1.00atm,O2=1.130atm,SO3=0atm (e) 2NO(g)+CI2(g)2NOCI(g) Kp=2.5103 ; initial pressures; NO=1.00atm,CI2=1.00atm,NOCI=0atm (f) N2(g)+O2(g)2NO(g) Kc=0.050 ; [N2]=1.00M,[O2]=0.200M,[NO]=1.00M