For the following reaction: A(g) + B(g) = C(g) Calculate the equilibrium constant K given the following information: The initial pressure of A is 4.421 bar and the initial pressure of B is 3.829 bar The equilibrium pressure of C is 1.699 bar.

For the following reaction: A(g) + B(g) = C(g) Calculate the equilibrium constant K given the following information: The initial pressure of A is 4.421 bar and the initial pressure of B is 3.829 bar The equilibrium pressure of C is 1.699 bar.

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

Identify the proper form of the equilibrium-constant expression for the equation N2 (g) + O2 (g) = 2NO(g) • View Available Hint(s) [NO] Ο Κ: [N2][O2] [NO]? O K: [N2][O2] 12 [N2][O2] O K = [NO]? 2[NO] Ο Κ- [N2][O2]
The formation of nitrogen monoxide from its elements has an equilibrium which favors reactants: N2 (g) + 02 (g) 2 NO (g) K, = 0.0290 at 2400°C If the initial partíal pressures of both reactant gases are 0.717 atm, what will be the equilibrium partial pressure of nitrogen monoxide? (A certain simplification is valid in solving this problem). 0.112 atm (A) (B) 0.0290 atm (C) 0.688 atm (D) 0.0563 atm (E) 0.0611 atm
A mixture of 0.009482 mol of CH4, 0.02708 mol of H2S, 0.02785 mol of CS2, and 0.02860 mol of H2 is placed in a 1.0-L steel pressure vessel at 3918 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g) 1 CS2(g) + 4 H2(g) At equilibrium 0.001533 mol of CH4 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2.Peq(CH4).Peq(H2S).Peq(CS2).Peq(H2).(b) Calculate KP for this reaction.KP.
Methane and water react to form carbon monoxide and hydrogen, like this: CH2(g)+H₂O(g) CO(g)+3H2(g) Suppose a mixture of CH 4, H2O, CO and H2 has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium to the right The pressure of CH4 will ? to the left Some CO is added. The pressure of H2O will ? (none) to the right The pressure of H2O will ? Some CH4 is removed. to the left The pressure of CO will ? (none)
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
Methane and water react to form hydrogen and carbon monoxide, like this: CH4(g) + H₂O(g) → 3 H₂(g) + CO(g) The reaction is endothermic. Suppose a mixture of CH4, H₂O, H₂ and CO has come to equilibrium in a closed reaction vessel. Predict what change, if perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. any, the perturbation change in composition The temperature is raised. The pressure of CH4 will The temperature is lowered. The pressure of H₂ will ? ? ↑ î shift in equilibrium O X to the right to the left (none) to the right to the left (none) Ś
A chemical engineer is studying the following reaction: H2(9)+Cl2(g) → 2 HCl(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.1. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, and lets the reaction begin. He then measures the inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel compound pressure expected change in pressure H, 2.75 atm t increase I decrease (no change) Cl, 4.00 atm t increase O I decrease O (no change) A HCI 2.10 atm O f increase OI decrease O (no change) H, 2.78 atm t increase I decrease O (no change) Cl, 4.03 atm t increase I decrease (no change) 2.06 atm t increase I decrease (no change) HCl H2 3.22 atm O f increase I decrease (no change) t increase I decrease (no change) Cl, 4.98 atm OI decrease O (no change) H CI 4.26 atm…
Consider the following equilibrium: N,0, (g) = 2NO, (3) AG' = 5.4 kJ Now suppose a reaction vessel is filled with 0.496 atm of nitrogen dioxide (NO,) at 137. °C. Answer the following questions about this system: O rise Under these conditions, will the pressure of NO, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,O,? In other words, if you said the pressure of NO, will tend to rise, can that O yes be changed to a tendency to fall by adding N,04? Similarly, if you said O no the pressure of NO, will tend to fall, can that be changed to a tendency to rise by adding N,0,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N,0, needed to reverse it. O atm Round your answer to 2 significant digits.
Carbon disulfide and oxygen react to form carbon dioxide and sulfur dioxide, like this: CS₂(g) +30₂(g) CO₂(g) +2SO₂(g) Suppose a mixture of CS2, O2, CO2 and SO₂ has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation Some O₂ is added. - Some CO₂ is removed. change in composition The pressure of CS₂ will The pressure of CO₂ will The pressure of CS₂ will The pressure of O₂ will ? ? ? ? ↑ ↑ ↑ ↑ shift in equilibrium X O OOO to the right to the left (none) to the right to the left O (none)
For the reaction 2 A(g) = B(g) + 3 C(g), we begin with only pure A(g) and the total pressure is 8.00 atm. We attain equilibrium. At equilibrium, the total pressure is 12.00 atm. What is the value of ∆G◦ for this reaction? The temperature is 25.0 ◦C throughout.
A chemical engineer is studying the following reaction: HCH;CO,(aq)+CH,NH,(aq) → CH;CO,(aq)+CH,NH,(2q) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.6. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction compound expected change in cor concentration concentration vessel HCH,CO, 0.96 M O T increase OI decrease O (no change) CH, NH, 0.88 M O f increase OI decrease O (no change) A CH,Co, 0.54 M O f increase OI decrease O (no change) CH,NH, 0.45 M O f increase OI decrease O (no change) HCH, CO, 0.88 M f increase OI decrease O (no change) CH,NH, 0.77 M O f increase OI decrease O (no change) B CH, Co, 1.09 M O increase OI…
A student ran the following reaction in the laboratory at 588 K: CO(g) + Cl₂(g) —COCI₂(g) When she introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 1.74 atm and the initial partial pressure of Cl2 was 0.951 atm, she found that the equilibrium partial pressure of COCI₂ was 0.685 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр =