Consider the following reaction:H2(g) + Cl2(g) 2 2 HCI(g)AH = -184.6 kJThe following graph represents a stress imposedon the system after equilibrium is initiallyestablished.HCLCl2He605040302010++10203040Concentration (mol/L) 4030201010203040Time (s)What stress occurred at 20 seconds in the graph?O Hydrogen chloride gas was addedChlorine gas was removedHydrogen gas was removedThe temperature was decreasedConcentration (m

According to Le - Chatelier's Principle, the reaction at equilibrium opposes the change due to the…

Consider the following reaction: H2(g) + Cl2(g) 2 2 HCI(g) AH = -184.6 kJ The following graph represents a stress imposed on the system after equilibrium is initially established. HCL Cl2 He 60 50 40 30 20 10 + + 10 20 30 40 Concentration (mol/L)

Consider the following reaction: H2(g) + Cl2(g) 2 2 HCI(g) AH = -184.6 kJ The following graph represents a stress imposed on the system after equilibrium is initially established. HCL Cl2 He 60 50 40 30 20 10 + + 10 20 30 40 Concentration (mol/L)

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

Ff.294.
Consider the equilibrium system described by the chemical reaction below. A mixture of gas containing only N₂ and H₂ is reacted in a vessel at high temperature. At equilibrium, the 5.0 M H₂, 8.0 M N₂, and 4.0 M NH 3 are present. Determine the initial concentrations of H₂ and N₂ that were present in the vessel. N₂(g) + 3 H₂(g) = 2 NH3(g) Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -2.0 0 2.0 5.0 -5.0 N₂(g) 8.0 1 6.0 + 4.0 -6.0 3 H₂(g) -4.0 10.0 2 NH3(g) RESET 11.0
11
Consider the following system at equilibrium: CH4(g) + 2H20(g) CO2(g) + 4H2(g) What change will cause the equilibrium to shift to form more CH4? Multiple Choice decrease (H2] increase (H20] decrease the volume of the reaction vessel increase (CH4] decrease [CO2] DELL
Which is true of a system at equilibrium when Kc < 1? O Equilibrium favors neither reactants or products Equilibrium favors products O Equilibrium favors reactants Equilibrium is shifting to the left Equilibrium is shifting to the right
Coal can be used to generate hydrogen gas (a potential fuel) by the following endothemic reaction (heat is on the reactant side of the equation). C (3) + H20 (g) = co (g) + H2 (g) If this reaction mixture is at equilibrium, predict whether each of the following will resuit in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. Part A adding more C to the reaction mixture the formation of additional hydrogen gas the formation of less hydrogen gas O no effect on the quantity of hydrogen gas
For the following reaction 2 SO2(g) + O2(g) <-> 2 SO3(g) + heat If the equilibrium situation is stressed by increasing the volume of the container, the reaction will shift toward a No change b Right or products c Left or reactants
Indicate whether or not product formation increases if the size of the reaction container is decreased for each of the following equilibrium systems. a) 4NH3(g) + 5O2(g) heat + 4NO(g) + 6H2O(g) b) heat + 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g)
Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. which will happen? the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease (b) The reaction mixture is cooled. the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease (c) The volume of the reaction vessel is reduced by 50%. (d) A catalyst is added to the reaction mixture. (e)…
Consider the following exothermic reaction system at equilibrium: N2(g) + 3H2(g) ⇒ 2NH3(g) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below: Note: Use I for increase, D for decrease, NC for no change Add N2(g) Remove H2(g) Add NH3(9) Add Ne(g) Increase the temperature (constant P) Decrease the volume (constant T) Add a catalyst Submit NH3 N₂ H2