Consider this reaction in a closed container. N₂O (9) 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 NO, 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.

Consider this reaction in a closed container. N₂O (9) 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 NO, 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.

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

Enter your answer in the provided box. Pure phosgene gas (COCI₂), 0.0220 mol, was placed in a 1.50-L container. It was heated to 720.0 K, and at equilibrium, the pressure of CO was found to be 0.503 atm. Calculate the equilibrium constant Kp for the reaction. Kp CO(g) + Cl₂(g) = COCI₂(g)
3. Please provide the correct answer choices for all parts to this chemistry problem.
SO₂ reacts with Cl₂ to form SO₂Cl₂. The equilibrium constant, Kp, for this reaction is 0.417 at 373 K. 4 SO₂(g) + Cl₂(g) =SO₂Cl₂(g) The standard enthalpy change for this reaction (AH°) is -67.2 kJ/mol. (a) Predict the effect on the production of SO₂Cl₂ when the temperature of the equilibrium system is increased. (b) Use the van't Hoff equation to estimate the equilibrium constant for this reaction at 449 K. Kat 449 K =
A mixture of 0.578 moles of carbon monoxide and 0.443 moles of oxygen was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium at a certain temperature. The equilibrium concentration of CO2 was 0.239 M. What is the value of Ke for this reaction at this particular temperature? CO(g) + O2(g) = CO2(g) Report your answer to three significant figures and do not include units.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction MnO4(aq) + 2 H2O(l)+3e MnO2(s)+4OH(aq) Br₂(1)+2e →>> 2 Br (aq) standard reduction potential E = +0.59 V 'red E = +1.065 V 'red Answer the following questions about this cell.
Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron/iron oxide catalyst. For the reaction: N₂(g) + 3H₂(g) → 2NH3(g) AH -92.22 kJ/mol At 300 °C the equilibrium constant for the reaction is 4.34 x 10-³. a) Is this reaction endothermic or exothermic? b) What effect would the following changes have on the equilibrium position. Write forward, reverse or no change: • Add some more nitrogen gas • Increase the volume of the reaction vessel • Decrease the temperature • Remove some hydrogen gas
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 100. L tank with 9.9 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.50 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significan digits. K = 0
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)
Coal can be used to generate hydrogen gas (a potential fuel) by the following endothemic reaction (heat is on the reactant side of the equation). C (3) + H20 (g) = co (g) + H2 (g) If this reaction mixture is at equilibrium, predict whether each of the following will resuit in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. Part A adding more C to the reaction mixture the formation of additional hydrogen gas the formation of less hydrogen gas O no effect on the quantity of hydrogen gas
A chemical engineer is studying the following reaction: BF3(aq) + NH3(aq) → BF3NH₂(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.9. с The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, 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 B с compound BF 3 NH3 BF₂NH₂ BE 3 NH3 BF, NH3 BF3 NH3 BF3NH₂ concentration 0.65 M 0.70 M 0.88 M 0.03 M 0.07 M 1.06 M 0.04 M 0.08 M 1.05 M expected change in concentration ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↓ decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease decrease ↓ decrease X (no change) (no change) (no change) (no change) (no change)…
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.
The equilibrium constant, Ko, for the following reaction is 10.5 at 350 K: 2CH,Cl2(g)= CH4(g) + CCI4(g) Calculate the equilibrium partial pressures of all species when CH,Cl,(g) is introduced into an evacuated flask at a pressure of 0.606 atm at 350 K. PCH;Cl2 = atm PCHA atm Pccla atm