At 25°C, gaseous SO,Cl, decomposes to SO, (g) and Cl, (g) to the extent that 12.5% of the original SO,Cl, (by moles) has decomposed to reach equilibrium. The total pressure at equilibrium is 0.900 atm. Calculate the value of K, for this system. (Hint: Set as P, the initial pressure of SO,Cl, and x the amount that has decomposed. Set 2 equations to solve for P, and x) Also PTotal = sum of the partial pressures

At 25°C, gaseous SO,Cl, decomposes to SO, (g) and Cl, (g) to the extent that 12.5% of the original SO,Cl, (by moles) has decomposed to reach equilibrium. The total pressure at equilibrium is 0.900 atm. Calculate the value of K, for this system. (Hint: Set as P, the initial pressure of SO,Cl, and x the amount that has decomposed. Set 2 equations to solve for P, and x) Also PTotal = sum of the partial pressures

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

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl₂, and NOCl 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?
Q3. At 298 K, F3SSF(g) decomposes partially to SF2(g). At equilibrium, the partial pressure of SF2(g) is 1.1X10-4 atm and the partial pressure of F3SSF is 0.0484 atm. (a) Write a balanced equilibrium equation to represent this reaction. (b) Compute the equilibrium constant corresponding to the equation you wrote. (c) Some SF2 (at a partial pressure of 2.3X10-4 atm) is placed in a closed container at 298 K with some F3SSF (at a partial pressure of 0.0484 atm). Enough argon is added to raise the total pressure to 1.000 atm. Calculate the initial reaction quotient for the decomposition of F3SSF to SF2.
Consider this reaction in a closed container. N₂O,(g) 2NO₂(g) = An equilibrium mixture is prepared at 298 K with these partial pressures: N₂O, = 3.476 atm, NO₂ 1.048 atm. Suddenly, just the NO₂ partial pressure is decreased by a factor of 2.6 In which direction do you predict the reaction will go to return to equilibrium? Calculate AG for this non-equilibrium mixture before any further reaction occurs. D Plus or minus 5% J/mol 3 Attempts Submit
1. Carbon dioxide reacts with carbon to give carbon monoxide according to the equation C(s) + CO,(g) 2CO(g) At 700°C, a 2.0-L sealed flask is found to contain at equilibrium 0.10 mol CO, 0.20 mol CO, and 0.40 mol C. Calculate the equilibrium constant K, for this reaction at the specified temperature.
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…
A chemical engineer is studying the following reaction: HCH;CO,(aq)+CH;NH,(aq) → CH;CO,(aq)+CH,NH,(aq) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.73. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. He then measures the composition of the mixture 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 compound concentration expected change in concentration vessel HCH;CO, 1.18 M f increase I decrease (no change) CH, NH, 0.97 M f increase OI decrease O (no change) A CH,CO, 0.39 M f increase O I decrease (no change) + CH,NH, 0.39 M f increase Ot decrease (no change) HCH,CO, 1.15 M f increase OI decrease O (no change) CH,NH, 0.88 M t increase I decrease (no change) В CH,CO, 0.86 M f increase OI decrease (no change) CH,NH,…
Consider the following reaction:COCl2(g) CO(g) + Cl2(g)If 8.62×10-3 moles of COCl2, 0.353 moles of CO, and 0.282 moles of Cl2 are at equilibrium in a 12.5 L container at 757 K, the value of the equilibrium constant, Kp, is .
A chem ngineer is studying the following reaction: 4 HCl(g)+O,(g) – 2 H,0(g)+2Cl,(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.0040. The engineer charges ("fillsf) four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. He then measures the co mixture 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 compound pressure expected change in pressure vessel HCl 8.71 atm Ot increase O! decrease O (no change) 02 8.13 atm O t increase OI decrease O (no change) H,0 3.63 atm Ot increase OI decrease (no change) I decrease (no change) Cl, 1.91 atm ease I decrease (no change) 7,61 atm t increase HCI I decrease O (no change) 7,86 atm O f increase 0, I decrease O (no change) 4.18 atm t increase H,0 I decrease (no change) t increase 2.46 atm Cl, I decrease O (no…
Consider the following reaction: NO(g) + SO3(g) = NO2(g) + SO2(g) A reaction mixture initially contains 0.639 M NO and 0.639 M SO3. Determine the equilibrium concentration of NO2 if K, for the reaction at this temperature is 0.0118. Enter the numerical value to three decimal places without units. Answer:
A chemical engineer is studying the following reaction: H₂(g) + Cl₂(g) → 2 HCl(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.83. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, and lets the reaction begin. He then measures the composition of the mixture 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 A C compound H₂ Cl₂ HCI H₂ CL₂ HCI H₂ CL₂ HCI pressure 4.00 atm 1.97 atm 3.36 atm 4.27 atm 2.82 m 3.84 atm 1.81 atm 3.69 atm expected change in pressure 1 increase O decrease decrease Of increase Of increase Ⓒ↓ decrease Of increase O decrease decrease O1 increase Ot increase O decrease Of increase O decrease Of increase O decrease decrease Of increase O (no change) (no change) O(no change) (no change) (no change) (no change) (no change) (no…