### Chemical Equilibrium Assessment#### The concentration of \( O_2 \) will:- ○ stay the same.- ○ increase.- ○ decrease.#### The concentration of \( SO_3 \) will:- ○ stay the same.- ○ increase.- ○ decrease.---The questions above pertain to changes in the concentration of oxygen (\( O_2 \)) and sulfur trioxide (\( SO_3 \)). These types of questions are typically used to assess understanding of chemical equilibrium and reactions, likely within the context of Le Chatelier's Principle or reaction kinetics.Each question asks you to predict whether the concentration of a given substance will remain the same, increase, or decrease under certain conditions. Proper understanding of the reaction mechanism and external influences (like temperature, pressure, and concentration changes) that could affect the equilibrium state is crucial for answering these questions. **Exothermic Chemical Reaction and Equilibrium Adjustment****Chemical Equation:**\[ 2 SO_2(g) + O_2(g) \leftrightarrows 2 SO_3(g) \ \text{(exothermic)} \]**Question:**Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after decreasing the temperature.**The concentration of \( SO_2 \) will:**- o increase.- o decrease.- o stay the same.

Temperature is one of the factors which affects the equilibrium and as per Le Chatelier's principle…

The chemical equation shown is an exothermic process. 2 SO, (g) + 0,(g)=2 SO,(g) exothermic Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after decreasing the temperature. The concentration of SO, will increase. decrease. stay the same.

The chemical equation shown is an exothermic process. 2 SO, (g) + 0,(g)=2 SO,(g) exothermic Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after decreasing the temperature. The concentration of SO, will increase. decrease. stay the same.

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 38A

See similar textbooks

Similar questions

12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial concentrations are [O3]=1.0106M,[NO]=1.0105M,[NO2]=2.5104M, and [O2]=8.2103M , is the system at equilibrium? If not, in which direction does the reaction proceed? (b) If the temperature is increased, as on a very warm day, will the concentrations of the products increase or decrease? (HINT: You may have to calculate the enthalpy change for the reaction to find out if it is exothermic or endothermic.)
How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.
The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative molecular picture that shows what this system looks like after the reactants are mixed in one of the boxes and the system reaches equilibrium. Support your answer with calculations.
. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
Explain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates are equal.
In the figure, orange fish are placed in one aquarium and green fish in an adjoining aquarium. The two tanks are separated by a removable partition that is initially closed. (a) Describe what happens in the first few minutes after the partition is opened. (b) What would you expect to see several hours later? (c) How is this system analogous to dynamic chemical equilibrium?
A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.
Complete the table below for the reaction 3A(g)+B(g)2C(g)
Tell what will happen to each equilibrium concentration in the following when the indicated stress is applied and a new equilibrium position is established. a. LiOH(s)+CO2(g)LiHCO3(s)+heat; CO2 is removed. b. 2NaHCO3(s)+heatNa2O(s)+2CO2(g)+H2O(g); The system is cooled. c. CaCO3(s)+heatCaO(s)+CO2(g); The system is cooled.
12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.