The following reaction is exothermic in the torward direction. Ni (s) + 4 CO (g) Ni(CO), (g) What affect would the following changes have on the equilibrium of the system? Indicate if the reaction would shift left, shift right, or no change would occur. Also give a well thought out reason for your answer. a. Increase in [CO] b. Increase in [Ni(CO)4] c. Increase in T d. Increase in pressure e. Decrease in T f. Decrease in pressure g. Addition of a catalyst h. Increase in [Ni]

The following reaction is exothermic in the torward direction. Ni (s) + 4 CO (g) Ni(CO), (g) What affect would the following changes have on the equilibrium of the system? Indicate if the reaction would shift left, shift right, or no change would occur. Also give a well thought out reason for your answer. a. Increase in [CO] b. Increase in [Ni(CO)4] c. Increase in T d. Increase in pressure e. Decrease in T f. Decrease in pressure g. Addition of a catalyst h. Increase in [Ni]

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

12. A 2.50 L vessel contains 1.75 mole N₂, 1.75 mol H₂ and 0.346 mole NH3. What is the direction of reaction needed to attain equilibrium at 401 °C? The equilibrium constant Kc for the reaction is 0.50 at this temperature. N₂(g) + 3H₂(g) 2NH3(g)
Keq for the reaction below is 0.680. Initially the concentration of carbon monoxide is 0.500 mol/L and chlorine is 1.00 mol/L. Determine the equilibrium concentrations of all entities. (This reaction will actually proceed to the LEFT!) COCl2 <---> CO(g) + Cl2(g)
Assuming the system is already at equilibrium, predict whether each of the following changes will cause the amount of CO2(g) to increase, decrease, or stay the same. 2 NaHCO3(s) <-> Na2CO3(s) + H2O(g) + CO2(g) H°= + 91.6 kJ/mol a. Increase the amount of NaHCO3(s)b. Increase the amount of Na2CO3(s)c. Increase the amount of H2O(g)d. Decrease the temperaturee. Addition of HCl (which catalyzes this reaction)f. Increase the volume of the reaction container
Given these initial concentrations: [SCN] = 0.000646 M, [Fe³+] = 0.000506 M, and [Fe(SCN)²+] = 0.000000 M, determine The value for K if the [Fe(SCN)2+] at equilibrium is 0.0000856 M. value for K: 1.09 X10-4 Incorrect
Given that Kp - 3.0 x 10 for the reaction: 2 CO(g) C(graphite) + CO2(g). what is the partial pressure of CO2(g) at equilibrium if initially 4.00 atm of CO(g) is in contact with graphite? MA. 0.0024.atm B. 0.0060 atm C.0.0048 atm D.0.0012 atm E. 0.0096 atm
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
For the reaction 2SO2(g) + O2g) 2SO3(2) If K. = 4.3 x 10° and the following concentrations are present: [SO2] = 0.010 M, [SO3] = 10 M, [O2] = 0.01 M. Which of the following statements is correct? A. The system is at equilibrium B. The system is not at equilibrium and is shifting from left to right C. The system is not at equilibrium and is shifting from right to left D. There is not enough information E. The system is at equilibrium and is shifting from left to right 3.
5. At 100.0°C, the equilibrium constant K for the reaction C(s) + 1/2O2(g) CO(g) is 2.58 x 10°. Write an equilibrium constant expression for this reaction. What is the numerical value of the equilibrium constant for each of the following reactions: 2.58x10 a. CO(g) C(s) + 1/2O2(g) at 100.0°C b. 4C(s) + 2O2(g) 4CO(g) at 100.0°C c. C(s) + 1/2O2(g) CO(g) at 125.0°C 3 [co] = [0₂]
64. Consider this reaction at equilibrium: 2 BRNO(g) = 2 NO(g) + Br2(8) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a. NO is added to the reaction mixture. b. BINO is added to the reaction mixture. c. Brz is removed from the reaction mixture.
Can you provide an explanation? And show the steps
Consider the reaction N2 (9) + 02 (e) + 2NO (e) that has K= 4 x 10-6 . Initially, 0.1 M N2 and 0.1 M O2 are placed in a container. What is the equilibrium concentration of NO? O 2.0 x 102 M O 1.4 x 102 M O 2.0 x 10-4 M O 1.0 x 10-4 M O 4.0 x 10-4 M
A 1.00 liter flask contained 0.24 mol NO2 at 700 K which decomposed according to the reaction 2 NO2(g) = 2NO(g) + O2(g). At equilibrium the amount of NO was measured to be 0.14 mol, what is the value of Kc? A. 9,6 x 103 B. 1.1 x 102 C. 9.8 x 102 D. 1,4 x 101 E. 5.7 x 103