### 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.

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

consider the following endothermic reaction in chemical equilibrium:A(g) + B (g) ⇋ C(g) + D(s)How many of the following changes will cause the reaction to shift to the right (in the direction of products) to re-establish equilibrium? adding some B(g) adding some D(s) increasing the volume of container cooling the reaction
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 125. I tank with 6.4 mol of sulfur dioxide gas and 14. mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 1.3 mol. Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K
Consider the equilibrium: 2N2O (g) + O2 (g) 4NO (g) 3.00 moles of NO (g) are introduced into a 1.00-Liter evacuated flask. When the system comes to equilibrium, 1.00 mole of N2O (g) has formed. Determine the equilibrium concentrations of each substance. Calculate the Kc for the reaction based on these data.
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 1.5 L flask with 1.0 atm of sulfur dioxide gas and 1.5 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.80 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K, x10 ?
A chemist is studying the following equilibirum, which has the glven equilibrium constant at a certain temperature: 2 NO(g) + Cl,(g) 2 NOCI(g) K.=9. x 106 9. He fills a reaction vessel at this temperature with 7.0 atm of nitrogen monoxide gas and 6.8 atm of chlorine gas. Use this data to answer the questions in the table below. O yes Can you predict the equilibrium pressure of NOCI, using only the tools available to you within ALEKS? x10 O no If you said yes, then enter the equilibrium pressure of NOCI at right. Round your answer to 1 significant digit. atm Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy Accessibilit M O hp
Carbon Tetrachloride can be produced by the following reaction: CS2 (g)+ 3 Cl2 (g)》S2 Cl2(g)+CCL4 (gas). Suppose 1.20 Mol of CS2 and 3.60 Mol of Cl2 were placed in a 1.0 L flask at an unknown temperature. After equilibrium has been achieved the mixture contains 0.76 Mol of CCl4. Calculate the Kc
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 125. L tank with 23. mol of sulfur dioxide gas and 56. mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 18. mol. Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K_ = [ x10
What happens to a reaction at equilibrium when more reactants are added to the system? The reaction proceeds to make more reactants. There is not enough information to determine what will happen. The reaction is unchanged. The reaction proceeds to make more products. The reaction will stop.
For the chemical equation SO2(g)+NO2(g)↽−−⇀SO3(g)+NO(g) the equilibrium constant at a certain temperature is 3.40. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.53 mol SO2(g) in order to form 1.10 mol SO3(g) at equilibrium. moles of NO2(g):
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 75.0L tank with 6.5 mol of sulfur dioxide gas and 29.mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 3.3 mol.Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits
What happens when a chemical reaches equilibrium? A The amounts of reactants and products remain constant because the reaction stops. B The reaction stops because the concentration of reactants is too low to sustain it. C The rate of the forward reaction is the same as the rate of the reverse reaction. D The reaction reverses so some of the products are converted back into reactants.
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 500. mL flask with 0.50 atm of sulfur dioxide gas and 3.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.050 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. -0 K = р x10 X Ś