The water gas shift reaction is represented by the equation and enthalpy change shown below:co + H20 = CO2 + H2AH'R = -41 kJ mol1For this question answer the following questions:i. What does the phrase 'equilibrium limited' mean?ii. What impact would increasing temperature have on the position of this equilibrium?i. How would adsorbing Co, on a solid adsorbent affect this equilibrium?Write your answer asi=ii =iii =

i) Equilibrium limited means a stable condition in which forces cancel one another i.e. if one of…

The water gas shift reaction is represented by the equation and enthalpy change shown below: co + H20 = co2 + H2 AH'R = -41 kJ mor1 For this question answer the folowing questions: i. What does the phrase 'equilibrium limited' mean? il. What impact wouid increasing temperature have on the position of this equilibrium? i. How would adsorbing CO2 on a solid adsorbent affect this equilibrium? Write your answer as

The water gas shift reaction is represented by the equation and enthalpy change shown below: co + H20 = co2 + H2 AH'R = -41 kJ mor1 For this question answer the folowing questions: i. What does the phrase 'equilibrium limited' mean? il. What impact wouid increasing temperature have on the position of this equilibrium? i. How would adsorbing CO2 on a solid adsorbent affect this equilibrium? Write your answer as

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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Consider the equilibrium: Sno, ()+ 20o ) Sn ()+ 200, le 5.0g of tin ( oide and 085 Mcarbon monoide were initially charged in a dosed reactor at room temperature and allowed to reach equilibrium. At equilibrium 0.65 Mof CO was measured. Calculate Ke for the equilibrium. O 0095 042 O022 11
17. When BaCO3 is first mixed with K3PO4 their concentrations are measured at: [BaCO3] = 0.968M and [K3PO4] = 0.745M. The reaction is allowed to progress until equilibrium is reached. At equilibrium [K₂CO3] = 0.804M. Calculate Keq. 3BaCO3(aq) + 2K3PO4 (aq) Ba3(PO4)2 (aq) + 3K₂CO3(aq) 18. For the following reaction, name 4 ways in which you can maximize the amount of product produced. CO(g) + 2H2(g) CH3OH(g) + heat
Answer the questions by absolute reason
Answer only no. 2, increased temperature and increased pressure
The initial concentrations of four species involved in an equilibrium are: [Cl2] = 1.40 M, [HCl] = 0.100 M, [O2] = 0.300 M and [H2O] = 0.500 M. Is the reaction at equilibrium? If not, in what direction must the reaction shift for the equilibrium to be reached? Set up Kc in terms of the initial amounts and x as done in class. Do not try to solve for x. Set it up so x is positive. 4 HCl(g) + O2(g) <====> 2 Cl2(g) + 2 H2O(g) Kc = 52 At equil? ______ Direction? _______ Expression ____________
43. Consider the reaction: Fe (aq) + SCN (ag) FeSCN2 (ag) A solution is made containing an initial [Fe*] of 1.0 x 10 M and an initial [SCN ] of 8.0 x 10 M. At equilibrium, [FESCN? ] = 1.7 x 10 M. Calculate the value of the equilibrium constant (K). %3D
Question 7. For the Haber process described by the following reaction. 2 NH3(g) N2(g) + 3 H2(g) The equilibrium constants as function of temperature are: Temperature (°C) Ke 95 12 4 0.1 0.05 (a) Determine AS° for the Haber process. a. -140 J/K.mol b. 142 J/K.mol c. 141 J/K.mol d. 140 J/K.mol 141 J/K.mol 227 300 327 427 527 e.
Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.
Instructions are in the attached image. Please answer a, b, and c. Thank you!
-cnow-owl.cengagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator-assignment-take S ot ts This question has multiple parts. Work all the parts to get the most points. [References] Phosphorus pentachloride decomposes at high temperatures. PCl5 (g) PC13 (g) + Cl2 (g) An equilibrium mixture at some temperature consists of 3.56 g of PCl5, 4.86 g of PCl3, and 3.59 g of Cl2 in a 1.00-L flask. a If you add 1.31 g of Cl2, how will the equilibrium be affected? shift left shift right no shift will occur pt pts 1 pt b What will the concentration of PC15 be when equilibrium is reestablished after addition of 1.31 g Cl₂? 1 pt [PC15] = mol/L 1 pt Submit 1 pt 1 pt Submit Answer Try Another Version 4 item attempts remaining ent 80 a F4 F2 F3 # SA % Cengage Learning | Cengage Technical Support F5 1 MacBook Air F6 A DII F7 F8 * A F9
Give good explanation Asap Thanks Sulfur dioxide reacts with carbon dioxide to form an equilibrium with sulfur trioxide and carbon monoxide, all gases. A mixture of 1.51 mole each of sulfur dioxide and carbon dioxide is placed in an 2.89 L container and allowed to reach equilibrium. If the equilibrium constant, Kc, is 2.27 at this temperature, what is the concentration of carbon dioxide at equilibrium? Keep extra significant figures during the calculation and round your answer to 3 decimal places.