Consider the equilibrium reaction: CaCO3(s) + H₂O(g) Ca(OH)2(s) + CO2(g) Which of the following statements is INCORRECT concerning the reaction above? AH = +69.1 kJ a. Adding H₂O(g) will lead to increased production of Ca(OH)2(s). b. Increasing the volume of the reaction vessel will not affect the reaction equilibrium. c. Increasing the temperature will favor the forward reaction. d. Increasing the amount of Ca(OH)2(s) in the system will favor the reverse reaction.

Consider the equilibrium reaction: CaCO3(s) + H₂O(g) Ca(OH)2(s) + CO2(g) Which of the following statements is INCORRECT concerning the reaction above? AH = +69.1 kJ a. Adding H₂O(g) will lead to increased production of Ca(OH)2(s). b. Increasing the volume of the reaction vessel will not affect the reaction equilibrium. c. Increasing the temperature will favor the forward reaction. d. Increasing the amount of Ca(OH)2(s) in the system will favor the reverse reaction.

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

For the reaction NO₂(g) + SO₂(g) →→ NO(g) + SO3(g), AH° = -41.8 kJ. How will the equilibrium concentration of NO be affected if: NO2 is removed from the container. O Concentration stays the same. O Concentration decreases. O Concentration increases. SO3 is added to the container. O Concentration increases. O Concentration stays the same. O Concentration decreases. The temperature of the reaction mixture is raised. O Concentration increases. O Concentration stays the same. O Concentration decreases. SO₂ is removed from the container. O Concentration stays the same. Concentration decreased. O Concentration increased. The pressure of the gas mixture is raised by compressing the volume to 3.00 L. O Concentration decreases. O Concentration stays the same. O Concentration increases.
Consider the equilibrium reaction. 2A+B↽−−⇀4C2A+B↽−−⇀4C After multiplying the reaction by a factor of 2,2, what is the new equilibrium equation? new equilibrium equation: 4A+2B↽−−⇀8C If the initial reaction contains 1.63 M A,1.63 M A, 1.15 M B,1.15 M B, and 2.95 M C,2.95 M C, calculate ?cKc for the new equilibrium reaction. Consider the equilibrium reaction 3A+B↽−−⇀2C3A+B↽−−⇀2C Write the equation for the reverse reaction. reverse reaction: 2C↽−−⇀3A+B If the equilibrium concentrations are 1.27 M A, 1.01 M B, and 2.45 M C,, calculate the value of the equilibrium constant of the reverse reaction.
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
2
4. For the reaction CH4(g) + 2 H2S(g) = CS2(g) + 4 H₂(g) Kc = 3.59 at 900 °C. For each of the following measured concentrations determine whether the reaction is at equilibrium. If not, in which direction will the reaction proceed to get to equilibrium? [CH] [H₂S] [CS₂] [H2] Expt 1 Expt 2 Expt 3 1.15 1.07 1.10 1.20 1.20 1.49 1.51 0.90 1.10 1.08 1.78 1.68
The chemical equation represents a reversible reaction. 3H2(9) + N2(9) # 2NH3(g) At equilibrium, 1 liter of a mixture of gases at 450°C contains 1.83 mol of hydrogen (H2), 0.793 mol of nitrogen (N2), and 1.72 mol of ammonia (NH3).What is the equilibrium constant for the reaction under these conditions? O A. 0.718 B. 0.609 O C. 1.39 O D. 0.159 96 5 6
Assume the following reaction system: H2 S(g) + Ci2(g) = S(s) + 2HCI(g) has arrived at a point of equilibrium. Predict how each of the following adjustments will affect the position of the object. equilibrium. Determine whether the equilibrium will shift to the right. to the left, or not at all (No effect). a. The system is supplemented with more chlorine gas. b. The system's sulfur content is reduced by half. C. An "acid scrubber" is placed to the container, which reacts with hydrochloric acid to remove it from the system. d. The activation energy is split in half thanks to a very efficient catalyst.
Consider the reaction: Heat + CaSO3(s) <----> CaO(s) + SO2(g) What change will cause an increase in the pressure of SO2 when equilibrium is reestablished? increasing the reaction temperature decreasing the volume of the container adding more CaSO3 removing CaO
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.
Consider the equilibrium reaction shown below: 3 NO2 (g) + H2O (l) ⇋⇋ 2 HNO3 (aq) + NO (g) If the total pressure on the system is increased (by compressing the volume), how will the concentration of the NO (g) be affected? Select one: a. The concentration of NO will increase. b. The concentration of NO will decrease. c. There will be no change in the concentration of NO.
Consider the reaction: A(g) = B(g) + C(g) Find the equilibrium concentrations of A, B, and C for each value of K. Assume that the initial concentration of A in each case is 1.0 M and that the reaction mixture initially contains no products. Make any appropriate simplifying assumptions. a. K. = 1.0 b. K. = 0.010 c. K. = 1.0 x 10-S