**Equilibrium and Reaction Shifts in the Haber Process**In the following reaction, will the concentration of hydrogen gas \([H_2]\) increase or decrease when equilibrium is reestablished after these stresses are applied?\[ \text{N}_2(g) + 3 \text{H}_2(g) \rightleftharpoons 2 \text{NH}_3(g) \quad \Delta H^\circ = -22 \, \text{kJ} \]- **NH\(_3(g)\) is added**: ___________- **Pressure is increased**: ___________- **N\(_2(g)\) is removed**: ___________- **Temperature is increased**: ___________**Explanation:**This problem is based on Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. Here, the equilibrium involves nitrogen (\(\text{N}_2\)), hydrogen (\(\text{H}_2\)), and ammonia (\(\text{NH}_3\)) with an exothermic reaction (\(-22 \, \text{kJ}\)). You'll need to assess whether each stress will increase or decrease hydrogen concentration upon reestablishing equilibrium.

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the pressure,…

In the following reaction, will the [H2] increase or decrease when equilibrium is reestablished after these stresses are applied? N2 (g) + 3 H2 (g) 2 NH3 (g) AH°= -22 kJ NH:(g) is added pressure is increased N2(g) is removed temperature is increased

In the following reaction, will the [H2] increase or decrease when equilibrium is reestablished after these stresses are applied? N2 (g) + 3 H2 (g) 2 NH3 (g) AH°= -22 kJ NH:(g) is added pressure is increased N2(g) is removed temperature is increased

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

Which of the following change will shift the equilibrium to the right for the following reaction? CaCO3(s) ------> CaO(s) + CO2(g) Group of answer choices Increasing CaCO3(s) Decreasing the pressure Decrease CaO(s) Increasing CO2 (g)
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
Nitesh
10 The equilibrium reaction of 2 moles of SOe) plus 1 mole of Oxe) produces 1 mole of SO3(g)- What is the equilibrium constant expression for this reaction. 2(g)
How will an increase in temperature affect the following equilibrium? How will a decrease in the pressure of the reaction vessel affect it? 302 (g) 203 (g) AH = 285 kJ An increase in temperature will shift the equilibrium to the left; a decrease in the pressure of the reaction vessel will shift the equilibrium to the right O An increase in temperature will shift the equilibrium to the right; a decrease in the pressure of the reaction vessel will shift the equilibrium to the right O An increase in temperature will shift the equilibrium to the right; a decrease in the pressure of the reaction vessel will shift the equilibrium to the left. An increase in temperature will shift the equilibrium to the left; a decrease in the pressure of the reaction vessel will not affect the equilibrium
Consider the following system at equilibrium where AH 2NOBr(g) 2NO(g) + Br₂ (9) O increases O decreases O remains the same The value of Qc O is greater than Ke is equal to Ke O is less than Ke If the VOLUME on the equilibrium system is suddenly increased at constant temperature: The value of Ke The reaction must O run in the forward direction to reestablish equilibrium. O run in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. = The number of moles of Br₂ will O increase O decrease O remain the same 16.1 kJ, and K = 6.50 × 10-³, at 298 K: -3
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
5) For the reaction shown below, at a particular time, the following concentrations are obtained: [CO] = 0.034 M, [CO2] = 3.6 x 10-17 M. Is this reaction at equilibrium? If not, which direction will the reaction proceed and what will the concentrations be at equilibrium? 2 CO (g) « C (s) + CO2 (g)Kc = 7.7 x 10-15
For the equilibrium shown below, assess whether the following mixture is at equilibrium. If the mixture is NOT at equilibrium, tell whether the reaction will form more reactant or more products to reach equilibrium. 2 CO2 (g) 2 CO (g) + O2 (g) Kc = 6.4 x 10-7 [CO2] = 5.3 x 10-2 M [CO] = 3.6 x 10-4 M [O2] = 2.4 x 10-3 M
What is the equilibrium-constant expression for the following reaction?N2O4 (g) <--> 2NO2 (g)
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
5.For the following equilibrium reaction: Energy + 2AB2 (g) 2 AB (g) + B2 (g) where K = 55 What will happen to the amount of B2 (increase, decrease or stay the same) if a catalyst is added some AB is removed temperature is increased pressure is increased the amounts of AB2 and AB are kept constant while the value of K is decreased