Consider the reaction below: H2 (g) + Cl2 2HCI (g) If the chemical reaction above were at equilibrium, what would be the effect of decreasing the concentration of H2? Both the forward and reverse reaction rates would decrease It would have no impact; the reaction would remain at equilibrium O The reaction would shift to the right, favoring the formation of product O The reaction would shift to the left, favoring the formation of the reactant(s)

Consider the reaction below: H2 (g) + Cl2 2HCI (g) If the chemical reaction above were at equilibrium, what would be the effect of decreasing the concentration of H2? Both the forward and reverse reaction rates would decrease It would have no impact; the reaction would remain at equilibrium O The reaction would shift to the right, favoring the formation of product O The reaction would shift to the left, favoring the formation of the reactant(s)

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

Suppose the reaction system: UO₂ (s) + 4HF (g) UF4 (g) + 2 H₂O (g) has already reached equilibrium. Predict the effect that each of the following changes will have on the direction of the reaction to reestablish equilibrium. Indicate whether the reaction will shift to the left, to the right, or no change. a. Additional HF is added to the system. b. The reaction is performed in a glass reaction container and the HF begins to react with the glass. c. Water vapor is added. d. The volume is increased.
In what direction, if any, would the equilibrium be shifted if the following changes were done on the reactions? CO (g) + H₂O(g) + CO₂(g) + H₂(g) CO₂ is added to reaction
Consider the reaction below at a particular temperature: CO2(g) + H2(g) CO(g) + H2O(g) When the reaction has finally reached equilibrium, O the concentrations of all reactants and products will remain constant. O the concentration of CO will be equal to the concentration of CO2. O only the forward reaction will be taking place. O adding a catalyst will cause more products to form
Use Le Chatelier's Principle to answer the questions about the following reversible reaction: N2O4 (g) ⇌ 2NO2 (g) You are observing this reaction in a closed container. What will happen to the equilibrium if you increase the pressure inside the container? Will it shift in the reverse direction to favor the formation of N2O4, will it shift forward to favor the formation of NO2, or will it stay the same?
Which is the appropriate description to show the effect of a catalyst on the reaction rate and equilibrium in a reversible reaction: Reactants › Products O• The rate of the forward reaction is increased. • The rate of the reverse reaction is decreased 0 •The equilibrium position is displaced to the right O • The rate of the forward reaction is increased. The rate of the reverse reaction is increased The equilibrium position is unchanged. • The rate of the forward reaction is increased. 0 •The rate of the reverse reaction is unchanged • The equilibrium position is displaced to the right • The rate of the forward reaction is unchanged. The rate of the reverse reaction is unchanged The equilibrium position is unchanged. Suppose that an exothermic reaction, Reactants < › Products, is at equilibrium. According to Le Chatelier's Principle, if the reaction temperature is increased, in which direction will the equilibrium be displaced? O The equilibrium will be displaced toward the…
The following gases are in equilibrium. CO (g) +H2O (g) H2 (2) + CO2 (g) + heat Select all of the ways that you could shift the reaction to the left. Lower the temperature O Add a reactant Add a product Increase the volume of the container O Decrease the volume of the container Raise the temperature Remove a reactant Remove a product
1) When a system is at equilibrium: A) the reaction rate of the forward reaction is equal to the rate of the reverse B) the reaction rate of the reverse reaction is small compared to forward C) the reaction rate of the forward reaction is small compared to the reverse D) the amount of product and reactant is exactly equal 2) What will be the equilibrium expression for this reaction? (DO NOT INCLUDE SOLID PRODUCTS, THEIR CONCENTRATION IS ALWAYS EQUAL TO 1.) 4 CuO (s) + CH4 (g) = CO2 (g)+ 4 Cu (s) + 2 H2O (g) A) [CuO]/[Cu] B) [CuO]4/[Cu]4 C) [Cu]4/[CuO]4 D) [CO2][H20]2/[CH4] 3) Which K value below corresponds to the system with the highest proportion of reactants? А) К 3D25 B) K = 0.067 C) K = 1.5 x 10-3 D) K 3D 1.2 х 103
For this reaction, the equilibrium constant, Kea, is 6.1 x 10-4 SO3 (g) - O2 (g) + 2SO3 (g) Select the most accurate statement. O the equilibrium favors reactants O the rate of the forwards reaction is very fastfast O at equilibrium, the reaction mixture will contain a lot of both reactants and products O the rate of the forwards reaction is very slow O the equilibrium favors products
For the following reaction at equilibrium, which of the changes below would cause the equilibrium to shift to the right and form more products? 2 NOBR(g) + 2 NO(g) + Br2(g) A H°n = 30 kJ/mol Increase the temperature Increase the container volume Remove some NO Add some NOBr
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
Consider the following reaction at equilibrium taking place in the gas phase: H2 + I2 double arrows 2 HI In what direction will the equilibrium shift if the volume of the container is decreased? Towards reactants Towards products Neither
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?