### Analyzing Chemical Equilibrium Shifts**Consider the following equilibrium reaction:**\[ \Delta + 2 \text{HF}_{(aq)} + \text{CO}_3^{2-}_{(aq)} \rightleftharpoons 2 \text{F}^-_{(aq)} + \text{H}_2\text{O}_{(l)} + \text{CO}_2_{(g)} \]**Predict which direction the equilibrium will shift (left, towards reactants or right, towards products) when you perform the following actions:**| **Action** | **Shift Left** | **Shift Right** ||--------------------------------------|----------------|-----------------|| Add HF to the reaction | | || Add Na₂CO₃ to the reaction | | || Add NaCl | | || Add KF to the reaction | | || Add CO₂ to the reaction | | || Remove CO₂ from the reaction | | || Remove HF from the reaction | | || **Increase pressure by reducing volume** | | || Cool the reaction mixture | | || Heat the reaction mixture | | |Each action affects the equilibrium position, causing it to shift left or right according to Le Chatelier's Principle. Fill in the corresponding columns with predictions based on the actions provided.

Le-Chatelier principle :According to Le-chatelier principle if any disturbance is introduced to…

Consider the following equilibrium reaction: A+ 2HF (aq) + CO2F 3(aq) Action Add HF to the reaction Add Na₂CO3 to the reaction Add NaCl Add KF to the reaction Add CO₂ to the reaction Remove CO₂ from the reaction Remove HF from the reaction (ay) Predict which direction the equilibrium will shift (left, towards reactants or right, towards products) when you perform the following actions: Increase pressure by reducing volume Cool the reaction mixture Heat the reaction mixture + H,O+COzg) Shift Left Shift Right

Consider the following equilibrium reaction: A+ 2HF (aq) + CO2F 3(aq) Action Add HF to the reaction Add Na₂CO3 to the reaction Add NaCl Add KF to the reaction Add CO₂ to the reaction Remove CO₂ from the reaction Remove HF from the reaction (ay) Predict which direction the equilibrium will shift (left, towards reactants or right, towards products) when you perform the following actions: Increase pressure by reducing volume Cool the reaction mixture Heat the reaction mixture + H,O+COzg) Shift Left Shift Right

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

4. Indicate whether each statement below is true or false, If a statement is false, rewrite it to produce a clo statement that is true. a) For a given reaction, the magnitude of the equilibrium constant is independent of temperature. b) If there is an increase in entropy and a decrease in enthalpy when reactants in their standard states are converted to products in their standard states, the equilibrium constant for the reaction will be negative. c) The equilibrium constant for the reverse of a reaction is the reciprocal of the equilibrium constant for the reaction itself
15
11
Consider the following exothermic reaction at equilibrium: N2 ( g ) + 2H2 ( 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. Complete the table with the terms increase, decrease, or no change.
Hydrofluoric acid and water react to form fluoride anion and hydronium cation, like this: + HF (aq)+H,O(1)→F (aq)+H,O¨(aq) At a certain temperature, a chemist finds that a 4.7 L reaction vessel containing an aqueous solution of hydrofluoric acid, water, fluoride anion, and hydronium cation at equilibrium has the following composition: compound amount HF 1.19 g H,0 846. g F 0.440 g H,0* 0.149 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0 |x10
Select all of the correct statements about equilibrium from the choices below. At equilibrium the rates of forward and reverse reactions are equal. As a reaction proceeds forward toward equilibrium the reactant concentrations drop. Reactants are transformed into products even at equilibrium. As a reaction proceeds forward toward equilibrium the product concentrations rise. At equilibrium all reactions stop. As a reaction proceeds forward toward equilibrium the forward rate constant drops.
Consider the following reaction at equilibrium in the gas phase: N2 + 3 H2 double arrows 2 NH3 + heat In which direction will the equilibrium shift if the reaction is cooled? Towards reactants Towards products Neither
Consider the following reversible reaction at equilibrium: CO(g) + Cl2(g) COCI,(g). Use Le Chatelier's principle to predict the effect of adding some Cl2(g) to the equilibrium system? the concentration of CO(g) increases the concentration of COC12(g) decreases the equilibrium system shifts to the right to restore equilibrium the equilibrium system shifts to the left to restore equilibrium no effect
Consider the following equilibrium: BaSO4 (s) Ba2+ (aq) + SO42 (aq); AH > 0 In which direction will the equilibrium shift (choose from: left, right, no effect) if: We add H2SO4, the equilibrium will shift to shift to equilibrium will shift to A We add heat, the equilibrium will A/ We add He(g), the Α
Consider the following exothermic reaction at equilibrium: N2 (g) + 2H2 (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. Complete the table with the terms increase, decrease, or no change
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
When nitrogen gas reacts with oxygen gas, nitrogen monoxide gas forms: N2(g) + O2(g) ⇋2NO(g) Initially, 0.40 mol of each reactant is placed into a 2.0 L container and equilibrium is established. If Keq=50.1 for the reaction, what are the equilibrium concentrations of all reactants and products? What two conditions are required, if we want to move reaction forward.