Ving equilibriium system involv- ing SO2, Cl2, and SO,Cl2 (sulfuryl dichloride): SO-(g) + Cl2(g) = SO,Cl2(g) 14.60 Predict how the equilibrium position would change if (a) Cl2 gas were added to the system; (b) SO,Cl2 were removed from the system; (c) SO2 were re- moved from the system. The temperature remains constant

Ving equilibriium system involv- ing SO2, Cl2, and SO,Cl2 (sulfuryl dichloride): SO-(g) + Cl2(g) = SO,Cl2(g) 14.60 Predict how the equilibrium position would change if (a) Cl2 gas were added to the system; (b) SO,Cl2 were removed from the system; (c) SO2 were re- moved from the system. The temperature remains constant

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...

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14.54 Heating solid sodium bicarbonate in a closed vessel establishes the following equilibrium: 2NaHCO3(s) = Na,CO3(s) + H,O(g) + CO2(8) What would happen to the equilibrium position if (a) some of the CO2 were removed from the system; (b) some solid Na,CO3 were added to the system; (c) some of the solid NaHCO3 were removed from the system? The temperature remains constant.
1.3 3 (i) In the Haber process for the production of ammonia, the following reaction occurs: 2 (g) + 3H₂(g) 2NH3(g) = DH is negative If the equilibrium concentrations for all the reactants and products at 600°C are: [N₂] = 0.40 mol/dm³, [H₂] = 1.20 mol/dm³ and [NH₂] = 0.20 mol/dm³ Construct an expression for K and calculate the numerical value of the equilibrium constant, K с (ii) At 500°C K. 0.062 mol 2dm. Compare this value to the one you calculated in 3(i) above and state whether the yield of ammonia is greater at 500°C or 600°C and briefly explain your choice.
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 =
Given the reaction shown below: Colg) + H;0(g) CO,(g) + H2(g) K-0.640 and with the following initial concentrations: (CO)-0.626 M (CO)= 0.981 M [H,O]= 0.5 M [Ha)= 0.95 M Select the statement that best describes the reaction. O The reaction is not at equilibrium. The reaction will shift to the left to reach equilibrium. O The reaction is at equilibrium. It will not shift in either direction. O The reaction is not at equilibrium. The reaction will shift to the right to reach equilibrium. O None of these. O The reaction is not at equilibrium. The reaction will not shift on its own to reach equilibrium.
A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant. A(s)↽−−⇀B(g)+C(g) Then, the container volume was doubled and equilibrium was re‑established. How many moles of A remain? Dont
4. What will be the effect of the following change on the given equilibrium system? system change result CH3OH is added to CH(g) +H20() =CH;OH(1) +H2(g) reaction container H2(g) + I2(g) = 2HI(g) an inert gas is added 2H2 (g) + O2 (g) = 2H20 (g) AH = -483.6 kJ/mol of O2 increase in temperature SnO2(g) + 2C(s) = Sn(s) + 2CO2(g) AH = + 360.0 KJ Pressure is decreased N2(g) + 3 H2(g) =2 NH3(g) AH = -92 kJ mol- the solution is cooled some AgNO; is added to the solution AgCl(s) = Ag*(ag) + CF(ag) N2(g) + 3 H2(g) =2 NH3(g) pressure is increased
A2
Write the Ke and Kp expressions for the following homogeneous equilibrium reactions: a) CO(g) + -O2(g) = CO2(g) b) 2CO,(g) = O,(g) + 2CO(g) c) N,0(g) = N2(g) + -0,(g)
(b) Consider the following endothermic reaction: COB12 (g) CO (g) + Br2 (g) Predict and explain the change in equilibrium position, if any, when the i) CO is removed ii) Brz is added ii1) temperature of the system is increased
References Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 688 K: 2HI(g) H2(g) + I½(g) When he introduced HI(g) at a pressure of 4.87 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.510 atm. Calculate the equilibrium constant, K,, he obtained for this reaction. %3D Submit Answer
Hh.53.
Which of the following stresses to a system at equilibrium cause an increase in the production of CH3OH ? CO(g)+ 2H2(g) → CH3OH(g) (a) H2 is added. (b) The volume is increased. (c) Argon is added. (d) Removing CO.