Consider the following system at equilibrium: C₂H₂(g) + Br₂(g) + 44 kJ <======> C₂H₂Br₂(g) Which of the following actions would cause the Ke to decrease? I. increasing the volume at constant pressure and temperature II. decreasing the volume at constant pressure and temperature III. increasing the temperature IV. adding bromine gas at constant temperature and pressure V. removing ethyne gas at constant temperature and pressure VI. decreasing the temperature ||| I and II O VI IV and V III and VI

Consider the following system at equilibrium: C₂H₂(g) + Br₂(g) + 44 kJ <======> C₂H₂Br₂(g) Which of the following actions would cause the Ke to decrease? I. increasing the volume at constant pressure and temperature II. decreasing the volume at constant pressure and temperature III. increasing the temperature IV. adding bromine gas at constant temperature and pressure V. removing ethyne gas at constant temperature and pressure VI. decreasing the temperature ||| I and II O VI IV and V III and VI

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

Consider the following reaction at 25oC: A2(g) + B2(g) 2 AB(g) Which of the following statements is true? A. K > 1; at equilibrium there is more products than reactants. B. K > 1; at equilibrium there is more reactants than products. C. K < 1; at equilibrium there is more products than reactants. D. K < 1; at equilib thisrium there is more reactants than prroducts.
For the reaction CaO(s) + CO2(g) CaCO3(s), the value of AH is -178 kJ/mol. Using Le Chatelier's principle, which of the following changes to the system will shift the equilibrium to the right? i) Increasing the amount of CaO. ii) Decreasing the volume of the container. iii) Increasing the temperature. iv) Decreasing the temperature O A. only ii and iii OB. only i & ii OC. all of them OD. only i & iv OE. only i & iii
Consider the following chemical equilibrium: C(s) + 2 H₂ (g) ⇒ CH₂(g) Now write an equation below that shows how to calculate K from K for this reaction at an absolute temperature T. You can assume I is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K -0 X 00
Consider the following system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K. N2(g) + 3H2(g) 2NH3(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc fill in the blank 1 A. increases. B. decreases. C. remains the same. The value of Q fill in the blank 2 A. is greater than Kc. B. is equal to Kc. C. is less than Kc. The reaction must: fill in the blank 3 A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The concentration of H2 will: fill in the blank 4 A. increase. B. decrease. C. remain the same.
following equilibrium reaction at 160.00 °C. If 0.420 atm of H2O2(g) is initially present, calculate the equilibrium partial pressures of H2(g), O2(g), and H2O2(g).
4. A. An important reaction in the commercial production of hydrogen is CO(g) + H2O(g) --><-- H2(g) + CO2(g) How will the system at equilibrium shift in each of the five following cases? (Use arrows or write "right" , "left" , or "no shift"). a. Gaseous carbon monoxide is removed b. In rigid reaction container, a catalyst is added. c. The temperature is decreased (the reaction is exothermic). d. The reaction container volume is doubled. e. Hydrogen gas is added. B. The equation above has a Kc value of 7.5 x 102. If 2.0 moles of each reactant and product are put into the same sealed 4.0 L container, determine the concentrations of all species present at equilibrium. Please answer A with sub parts and B.
The following reaction is product-favored at equilibrium at room temperature. C,H2 (g) + H2 (g) → C,H4 (g) Will raising or lowering the temperature make it reactant-favored? Raising the temperature can make it reactant-favored. O Lowering the temperature can make it reactant-favored. O Neither raising nor lowering the temperature can make it reactant-favored.
` Effect of ΔT on Equilibrium Describe the difference in pressure in the ice-cold bottle and the hot bottle of a carbonated beverage. Use Le Chatelier's principle to explain the observation. What evidence is there of an equilibrium between aqueous CO2 and gaseous CO2?
For the equilibrium system below, which of the following would result in an increase in the quantity of H₂(g)? H₂(g) + 12(g) 2HI(g) + 65 kJ ос removing some I₂(g) and removing some HI(g) removing some HI(g) removing some 1₂(g) decreasing temperature removing some HI(g) and decreasing temperature
For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25°C, it is found that the partial pressure of C is 0.270 atm. What is AG° for this reaction? (R = 8.314 J/mol · K). kJ/mol 1 3 4 C 7 8 9 +/- x 100 + 2.