**Chemical Equilibrium Problems**1. **Consider the reaction:** \[ 2 \text{NO} (g) + \text{Br}_2 (g) \rightleftharpoons 2 \text{NOBr} (g) \] - \( K_p = 28.4 \) at 298 K. - In a reaction mixture at equilibrium, the partial pressure of NO is 0.142 atm and Br\(_2\) is 0.166 atm. **Question:** What is the partial pressure of NOBr in this mixture?---2. **Consider the reaction:** \[ \text{SO}_2\text{Cl}_2 (g) \rightleftharpoons \text{SO}_2 (g) + \text{Cl}_2 (g) \] - \( K_p = 2.91 \times 10^3 \) at 298 K. - In a reaction at equilibrium, the partial pressure of SO\(_2\) is 0.180 atm and that of Cl\(_2\) is 0.375 atm. **Question:** What is the partial pressure of SO\(_2\)Cl\(_2\) in this mixture?---**Explanatory Notes:**- These problems involve using the equilibrium constant (\( K_p \)) to find unknown partial pressures in gaseous chemical reactions.- Remember to apply the equilibrium constant expression to relate the partial pressures of reactants and products for the reaction in question.- Ensure correct units are used when calculating and referencing pressures.

Answered: Image /qna-images/answer/6ec864e2-6ad6-4ce0-9b93-812c2b9af6ad.jpg

1. Consider the reaction 2 NO (g) 2 NOBr (g) Kp = 28.4 at 298 K. In a reaction mixture at equilibrium, the partial pressure of NO is 0.142 atm and Br2 is 0.166 atm. What is the partial pressure of NOBr in this mixture? 2. Consider the reaction SO₂Cl2 (9) Kp = 2.91 x 10³ at 298 K. + Br₂ (g) SO₂ (g) + Cl2 (g) In a reaction at equilibrium, the partial pressure of SO₂ is 0.180 atm and that of Cl₂ is 0.375 atm. What is the partial pressure of SO₂Cl2 in this mixture?

1. Consider the reaction 2 NO (g) 2 NOBr (g) Kp = 28.4 at 298 K. In a reaction mixture at equilibrium, the partial pressure of NO is 0.142 atm and Br2 is 0.166 atm. What is the partial pressure of NOBr in this mixture? 2. Consider the reaction SO₂Cl2 (9) Kp = 2.91 x 10³ at 298 K. + Br₂ (g) SO₂ (g) + Cl2 (g) In a reaction at equilibrium, the partial pressure of SO₂ is 0.180 atm and that of Cl₂ is 0.375 atm. What is the partial pressure of SO₂Cl2 in this mixture?

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

Similar questions

b For the reaction H2(g) + Br2(g)→ 2HB1(g) Kp = 3.4 x 104 at 1493 K. What is the value of K, for the following reaction at 1493 K? 2HB1(g) H2(g) + Br2(g) K"p=
Consider the reaction N2(g) + O2(g) = 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.28, 0.26, and 0.025 atm, respectively, at 2200°C, what is Kp?
7. Given the reaction, N2 (g) + O2 (g) = 2 NO (g), Ke = 2.5 x 103 at 2130°C, decide whether the following mixture is at equilibrium or if a net forward or reverse reaction will occur. [NO] = 0.0050 M, JO2] = 0.25 M, and [N2] = 0.020 M.
Consider the following reaction where K. = 10.5 at 350 K: 2 CH;Cl2 (g)=CH4 (g)+ CCI4 (g) A reaction mixture was found to contain 1.10x10-2 moles of CH,Cl, (g), 4.63×10-2 moles of CH4 (g), and 3.70×10² moles of CCl (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: v 1. In order to reach equilibrium CH,Cl,(g) must be produced. v 2. In order to reach equilibrium K, must decrease v 3. In order to reach equilibrium CH, must be consumed. v 4. Qc is greater than K. 5. The reaction is at equilibrium. No further reaction will occur. T
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
For the equilibrium N2O4(g) <----> 2 NO2(g), at 298 K, Kp = 0.15. For this reaction system, it is found that the partial pressure of N2O4 is 3.7 × 10^–2 atm at equilibrium. What is the partial pressure of NO2 at equilibrium?
12.) A sample of ammonia gas was allowed to come to equilibrium at 400 K.2NH3(g) = N2(g) + 3H2(g) At equilibrium, the mixture contained to following concentrations: [H2] = 0.0283 M, [N2] = 0.00944 M,[NH3] = 0.101 M. What is Kp at this temperature?
Q2
Nitrogen dioxide reacts to form dinitrogen tetroxide as follows: 2 NO2 N₂04 (g) At 150 °C, Kp = 4.51. If one starts with 10.0 atm NO2 (g), what is the equilibrium pressure (in atm) of N₂O4 (g)?
3. Consider the reaction Br2 (g) + Cl2 (g) 2 BrCl (g) Kp = 1.11 x 104 at 150 K. A reaction mixture initially contains a Br2 partial pressure of 0.993 atm and a Cl2 partial pressure of 0.967 atm at 150 K. Calculate the equilibrium partial pressure of each reactant and product. 4. Consider the reaction CO₂ (g) + H2 (g) A reaction mixture initially contains a CO partial pressure of 1.768 atm and a H₂O partial pressure of 2.324 atm at 2000 K. Calculate the equilibrium partial pressures of each reactant and product. CO (g) + H₂O (g) Kp = 0.0611 at 2000K.
At 900 K, the following reaction has Kp = 0.345: 2 SO2(g) + O2(g) ⇋ 2 SO3(g). In an equilibrium mixture, the partial pressure of SO2 and O2 are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3 in the mixture?
An empty steel container is filled with 3.10 atm of H₂ and 3.10 atm of F2. The system is allowed to reach equilibrium. If Kp = 0.450 for the reaction below, what is the equilibrium partial pressure of HF? H₂ (g) + F₂ (g) → 2 HF (g)