15.23 The equilibrium constant for the reaction 2 NOBr (g) 2 NO(g) + Br2(g) 2 is K 1.3 x 10 at 1000 K. (a) At this temperature does the equilibrium favor NO and Br2, or does it favor NOBR? (b) Calculate K for 2 NOBr(g) = 2 NO(g ) + Br2(g). (c) Calculate K, for NOBr(g) NO (g) +Br2(g).

15.23 The equilibrium constant for the reaction 2 NOBr (g) 2 NO(g) + Br2(g) 2 is K 1.3 x 10 at 1000 K. (a) At this temperature does the equilibrium favor NO and Br2, or does it favor NOBR? (b) Calculate K for 2 NOBr(g) = 2 NO(g ) + Br2(g). (c) Calculate K, for NOBr(g) NO (g) +Br2(g).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: NO(g) and 0.160 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration…

A: From the given values, 2NO Br2 2NOBr I 0.218 0.160 0 C -2x -x +2x E 0.218-2x 0.160-x 2x…

Q: At a certain temperature, the equilibrium constant, Kc , is 0.00324 for the reaction…

A: A)The Kc expression for given reaction is as follows,

Q: At 100 °C, the equilibrium constant for the reactionCOCl21g2 ∆ CO1g2 + Cl21g2 has the value Kc =2.19…

A: For a reversible reaction at any stage other than the equilibrium, the ratio of the products of the…

Q: At 25 °C and at 1 atm, the partial pressures in an equilibrium mixture of N2O4 and NO2 are PN2 O4 =…

A: Given: Temperature is

Q: 2.) Formamide decomposes at high temperature. (a) If 0.186 mole of formamide (HCONH2) dissociates in…

A: The equilibrium reaction given is, a) Given: Moles of HCONH2 taken = 0.186 mol. Volume of flask =…

Q: The equilibrium system 2SO2(g)+ O2(g) = 2S03(g) is an exothermic reaction. Which change will result…

A: The correct option is:

Q: 15.109 The reaction NO(g) + NO₂(g) = N₂O3(g) takes place RAN in the atmosphere with K = 13 at 298 K.…

A: We know that Partial pressure of gas is according to Daulton's law of partial pressureHence, initial…

Q: A student ran the following reaction in the laboratory at 440 K: PC15 (9) PC13(g) + Cl₂(g) When she…

A: The given equilibrium reaction is .The initial moles of PCl5 is 1.58 mol.The volume of the container…

Q: A student ran the following reaction in the laboratory at 271 K: 2NO(g) + Br2(g) = 2NOBR(g) When she…

Q: A student ran the following reaction in the laboratory at 666 K: 2NH3(9) ? N₂(g) + 3H₂(g) When she…

Q: Phosphorus trichloride and chlorine gas react to form phosphorus pentachloride: PCh (g) + Cl, (R) O…

A: Using ICE table PCl3 Cl2 PCl5 Initial 1.0 M 2.0 M 0 Change x x x Equilibrium 1.0 -x…

Q: An equilibrium mixture is 0.146 M NOBr, 0.363 M NO, and 0.321 M Br2. (a) What is the value of Kc…

A: Given , Equilibrium concentration : NOBr = 0.146 MNO = 0.363 MBr2 = 0.321 M

Q: Phosphorous pentachloride decomposes according to the reaction PCI,(g) = PCI, (g) + Cl,(g) A 10.7 g…

A: Phosphorus pentachloride decomposes to give phosphorus trichloride and chlorine gas. The initial…

Q: Consider the reaction of NH, and I, to give N, and HI. 2 NH, (g) + 3 1, (g) N,(g) + 6 HI(g) K Using…

A: Equilibrium constant is the ratio between reactant and product concentration at equilibrium state.…

Q: For the reaction, N2(g) + O¿(g) = 2NO(g) K, is 0.01 at 2000 °C. After this system has established…

Q: Consider the reaction of NH, and I, to give N, and HI. 2 NH, (g) + 3 L, (g) N,(g) + 6 HI(g) K Using…

A: For a set of reactions, if we add the reaction together then the equilibrium constants of the two…

Q: A student ran the following reaction in the laboratory at 224 K: 2NOBr(g) 2NO(g) + Br₂ (9) When she…

A: Given, 2NOBr(g) ⇌2NO(g) + Br2(g) Initially, moles of NOBr(g) = 0.187 moles Volume of the container…

Q: The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600K.

A: Given chemical reaction is COCl2(g) <===> CO(g) + Cl2(g) Equilibrium constant Kc = 1.29×10-2…

Q: 5. For the equilibrium Br2(g) 2 Br (g) at 1000 K, K = 4.55. In a 1.00-L flask, 0.012 mol of Br₂ is…

Q: A student ran the following reaction in the laboratory at 448 K: PC15 (9) PC13 (g) + Cl₂ (g) When…

Q: Phosphorous pentachloride decomposes according to the reaction PCI, (g) = PCI,(g) + Cl,(g) A 10.1 g…

A: Given PCl5 (g) <----> PCl3(g) + Cl2(g) Initial Amount of PCl5 = 10.1 g

Q: The equilibrium constant for the following reaction is 6.47x10-2 at 396 °C. So2Cl2(g) sO2(g) +…

A: given, for a reaction: SO2Cl2(g) ⇔ SO2(g) + Cl2(g) 1 equilibrium constant, K =…

Q: NH3 is determined to be 2.00 M. below. 3) 2NH3(8)

Q: 9.19) What is the Ke for the equilibrium reaction of carbon monoxide gas reacting with hydrogen gas…

Q: A student ran the following reaction in the laboratory at 1082 K: 2 S03 (g)=2 SO, (g) + 02 (9) When…

Q: The equilibrium constant for the following reaction is 21.3 at 367 °C. K= 21.3 at 367 °C CO(g) +…

Q: The equilibrium constant, Kc, for the following reaction is 1.19x10-2 at 335 K. 2NOBr(g) 2NO(g) +…

A: Since,Equilibrium constant or Kc is the ratio of the equilibrium concentrations of product over…

Q: Consider the equilibrium4NO2(g) + 6H2 O(g) ⇌ 4NH3(g) + 7O2(g)(a) What is the expression for the…

A: A reaction system approaches equilibrium when there is a change in concentrations (or) pressure of…

Q: Given K = 0.71 at 45 oC for the reaction... A(g) + B(g) C(g) and K = 7.10 at 45 oC…

Q: H2 + 12 > HI for which the equilibrium constant K = 580 at 150 C. Suppose 0.300 mol of H2 (g) and…

A: Given: The reaction is as follows: H2 + I2 -------------------> 2HI. The…

Q: Write the equilibrium constant expression for each of the following reactions and classify the…

A: Homogeneous reaction , any of a class of chemical reactions that occur in single phase i.e. solid ,…

Q: (a) CaCO,(s)²Ca²*(aq) + CO,²-(aq) (b) Mg,(PO,);(9) =3 Mg²"(aq) + 2 PO,' (aq) (c) CO(g) +…

Q: Consider the following reaction, A <--->2B Kc= 2.56 X 10^-6 If 4.00 M of A is heated to 500 K,…

A: The equilibrium constant for the given reaction is low thus reaction proceeds very slowly. The…

Q: 2. At a certain temperature and a total pressure of 1.4 atmosphere, the partial pressure of an…

A: Equilibrium constant aA+bB⇔cC+dD Equilibrium constant for the above reaction can be written as;…

Q: Ammonia is produced by the following reaction: N,(g) + 3H2(g) = 2NH3(g) In an experiment, 1.00 mol…

Q: The dehydrogenation of benzyl alcohol to make the fla- voring agent benzaldehyde is an equilibrium…

Q: At 1.0 x 103 K, Kp = 1.85 for the reaction : SO2(g) + ½O2(g) ó SO3(g)(a) What is the value of Kp…

A: SO2(g)+1/2O2=>SO3(g). Kp=1.85. (Equation -1) T=1×10^3K a)…

Q: Suppose a 500. mL flask is filled with 1.6 mol of H,0, 0.30 mol of CO, and 0.80 mol of H,. The…

A: Answer: 0.23 M

Q: Consider the equilibrium 4NH; (g) + 502 (g) ANO (8) + 611, 0(8) Which one of the followings will…

A: The objective of the question is to determine which of the given options will shift the equilibrium…

Q: 6. Given a reaction below. 2NO(g) + 2H:(8) N:(g) + 2H₂O(g) At initial, 0.05 M of NO was mixed with…

A: Nitrogen oxide reacts with hydrogen to form nitrogen and water. The equation for the balanced…

Q: Write the expressions for K, for the following reactions. In each case indicate whether the reaction…

A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.…

Q: At 457K NO2(g) was evacuated to a reaction chamber until the pressure was 0.0539 atm. When…

A: Given equilibrium is 2NO2(g) ↔ 2NO(g) + O2(g) Temperature = 457 K Initial pressure…

Q: A student ran the following reaction in the laboratory at 545 K: COC12 (g) CO(g) + Cl₂ (g) When she…

Q: . The Water Gas equilibrium, co (8) + H20 (g) = CO2 (g) + H2 (g) has a equilibrium position when…

Question

15.23 The equilibrium constant for the reaction
2 NOBr (g)
2 NO(g) + Br2(g)
2
is K 1.3 x 10 at 1000 K. (a) At this temperature does
the equilibrium favor NO and Br2, or does it favor NOBR?
(b) Calculate K for 2 NOBr(g) = 2 NO(g ) + Br2(g).
(c) Calculate K, for NOBr(g) NO (g) +Br2(g).

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

A student ran the following reaction in the laboratory at 1083 K: 2503(g) 2sO2(g) + 02(g) When she introduced 7.36x10-2 moles of SO3(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 4.23x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc II
C and D
A student ran the following reaction in the laboratory at 251 K: 2NO(g) + Br2(9) 2NOBR(g) When she Introduced 0.248 moles of NO(g) and 0.171 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBR(g) to be 0.209 M. Calculate the equilibrium constant, Ke she obtalned for this reaction. K =
(a) Formulate the equilibrium expression for the endo- thermic reaction AgCl-NH3(s) = A£CI(s) + NH3(g) (b) What is the effect on PNH, at equilibrium if addi- tional AgCl(s) is added? (c) What is the effect on PNH, at equilibrium if addi- tional NH3(g) is pumped into or out of the system, provided that neither of the two solid phases shown in the chemical equation is completely used up? (d) What is the effect on PNH; of lowering the temperature?
An important step in the industrial production of hydro- gen is the reaction of carbon monoxide with water: CO(g) + H2O(g) = CO2(g) + H2(g) (a) Use the law of mass action to write the equilibrium expression for this reaction. (b) At 500°C, the equilibrium constant for this reaction is 3.9. Suppose that the equilibrium partial pressures of CO and H,O are both 0.10 atm and that of CO, is 0.70 atm. Calculate the equilibrium partial pressure of H2(g).
please provide detailed solution and give the explanation of the concept.... A student ran the following reaction in the laboratory at 656 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.62×10-2 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 0.118 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = ?
The equilibrium constant for the following reaction is 260 at -1 °C. 2 NO(g) + Br₂(g) 2 NOBr(g) K 260 at -1 °C - Calculate the equilibrium constant for the following reactions at -1 °C. (a) 2 NOBr(g) (b) NOBr(g) ? 2 NO(g) + Br₂(g) NO(g) + 1/2 Br₂(g) K = K =
A student ran the following reaction in the laboratory at 541 K: COC12 (9) CO(g) + Cl₂ (g) When she introduced 0.849 moles of COC1₂ (g) into a 1.00 liter container, she found the equilibrium concentration of COC1₂(g) to be 0.816 M. Calculate the equilibrium constant, Ke, she obtained for this reaction. Ke =
In an experiment, gaseous C2H4 and H2O, at 25 mmol each, were mixed in a 50-mL flask that contains 2.5 mmol of C2H6. (a) Determine the equilibrium constant if, at equilibrium, 16 mmol of C2H6 was present. C2H4(g) + H2O(g) ⇋ C2H6(g) + O2(g) At one point of the experiment, it was found that 9.7 mmol C2H4, 7.5 mmol H2O, 21.9 mmol C2H6 and 16.4 mmol O2 were present in the flask. (b) At what direction should the reaction proceed to achieve equilibrium? Support your answer with calculations and explain your answer in not more than 3 sentences.
A student ran the following reaction in the laboratory at 1097 K: 2SO3(g)2SO2(g) + O2(g) When she introduced 0.0921 moles of SO3 (g) into a 1.00 liter container, she found the equilibrium concentration of O₂ (g) to be 0.0198 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
A student ran the following reaction in the laboratory at 1152 K: 2502(g) + 02(g) = 2503(g) When she introduced 7.99x102 moles of so, (g) and 7.30x102 moles of 02(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 4.51×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. K =
Compare the following two reactions ("A" and "B"), with two different equilibrium constants, K: (A) Cl2 (g) + H2 (g) = 2HCI (g) K = 0.29 (B) I2 (g) + H2 (g) = 2HI (g) K = 1.6 x 1033 %3D Which of the following statements is correct? O Reaction "A" will proceed faster because the equilibrium constant, K, is larger O Reaction "B" will proceed faster because the equilibrium constant, K, is larger O Reaction "A" favors the production of products. O Reaction "B" favors the production of products. O None of these statements are correct.