Gaseous sulfur dioxide reacts with oxygen to from gaseous sulfur trioxide. a. Write a balanced chemical equation for this reaction. b. At some temperature, the equilibrium constant for this reaction is 16. If 1.0 mole of sulfur dioxide, 1.8 mole of oxygen, and 4.0 mole of sulfur trioxide are placed in a 2.0 L flask at this temperature will the reaction proceed to the products or to the reactants? c. Compare the amount of reactants and products at equilibrium to the amount of reactants and products added to the flask in part b.

Gaseous sulfur dioxide reacts with oxygen to from gaseous sulfur trioxide. a. Write a balanced chemical equation for this reaction. b. At some temperature, the equilibrium constant for this reaction is 16. If 1.0 mole of sulfur dioxide, 1.8 mole of oxygen, and 4.0 mole of sulfur trioxide are placed in a 2.0 L flask at this temperature will the reaction proceed to the products or to the reactants? c. Compare the amount of reactants and products at equilibrium to the amount of reactants and products added to the flask in part b.

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

Related questions

Q: If calcium hydroxide (Ca(OH)2) and carbon dioxide (CO2) are in a solution and react to form solid…

A: The complete reaction is Ca(OH)2 (aq) + CO2 (aq) -> CaCO3 (s) + H2O (l) The given reaction is…

Q: 19. When the equilibrium constant is relatively small, what is true of the equilibrium? A. It is…

A: Please find the attached sheet.

Q: The synthesis of ammonia from nitrogen and hydrogen is an important industrial process for producing…

Q: 6. When solid barium fluoride is in equilibrium with its ions, the ratio of fluoride ion to barium…

Q: Consider the following exothermic reaction: 4 NH3 (g) + 5 O2 (g) ⇋⇋ 4 NO (g) + 6 H2O…

A: Pressure effect- Reaction shift to side with less no of moles, So product have 4 gaseous mole and…

Q: Nitrogen gas (N2) reacts with hydrogen gas (H₂) to form ammonia (NH3). At 200°C in a closed…

Q: Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using…

A: The value of equilibrium constant indicates towards the extent to which the reaction has occurred.…

Q: Which of the following is true about a reversible reaction at its equilibrium? a. The…

A: Equilibrium is that state of any reaction where we have no net consumption of reactants and no net…

Q: a. What is the name of HOCI? b. Write the equilibrium-constant expression (K) for the given…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: 11. Which of the following is true for a chemical reaction at equilibrium? The forward reaction goes…

A: Since, In chemical reaction, Equilibrium constant is the ratio of rate of forward reaction to the…

Q: Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its…

A: Given data : Volume of system = 50.0 L moles of ammonia = 4.6 mol moles of oxygen gas = 4.5 mol…

Q: 6.Study the reaction. CaO (s)+H2O (l)⇌Ca(OH)2 (s)+heat How does the equilibrium position react if…

A: The chemical equation : CaO(s) + H2O(l) <----> Ca(OH)2(s) + Heat. If temperature decrease then…

Q: QUESTION 6 Chemical Equilibrium Which statement is true about a chemical reaction which is at…

A: The question is based on the concept of chemical equilibrium. we need to identify the correct…

Q: What happens when a chemical reaction reaches equilibrium? A. The rate of the forward reaction and…

A: The correct option has to be identified when a chemical reaction reaches equilibrium has to be…

Q: Consider the following equilibrium: NF3 (g) + F2 (g) = NF5 (g) AH = -560 kJ/mol According to the Le…

A: To solve this problem use le chatelier's principle.

Q: 1.a. A sample of nitrogen gas has reacted with oxygen gas to form an equilibrium to produce nitrogen…

A: a. The balanced chemical equation and an equilibrium expression for the reaction :

Q: Consider the chemical system CO+ Cl COC2; K=4.6 x 10° L/mol. How do the equilibrium concentrations…

A: Option: a. They reactants are much smaller than the products.

Q: For the equilibrium reaction: 2 NOCl(g) 2 NO(g) + Cl2(g) 4.00 mol NOCl was placed in an otherwise…

Q: At a certain temperature, 0.3211 mol of N2 and 1.741 mol of H2 are placed in a 1.50 L container.…

A: Given that : Initial moles of N2 = 0.3211 mol Initial mole of H2 = 1.741 mol The volume of container…

Q: In the human body, the enzyme carbonic anhydrase catalyzed the interconvension of CO2 and HCO3- by…

Q: A 4.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into…

Q: 16. Consider this equilibrium, established in a sealed 2.0-L flask at 25°C: N,0,(g) = 2 NO,(g) AH° =…

Q: Thich statement(s) characterize(s) a emical system at equilibrium? I. The rate of the forward…

Q: Which of the following is an endergonic process? a. exothermic reactions b. endothermic reactions…

A: The endergonic process is endothermic reaction where energy is absorbed

Q: Why did heating cause the equilibrium to shift? In which direction did the equilibrium shift?…

Q: A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into…

A: Initial moles of sample A are 6.00 molesVolume is 1.00 LEquilibrium concentration of B = 1.40 M

Q: Decide whether each of the following statements is true or false. If false, change the wording of…

A: " Since you have posted a question with multiple sub-parts , we will solve first three sub-parts for…

Q: 7. The following exothermic reaction has an established chemical equilibrium. CHa(g) + 2H2S(g)→…

Q: A container is initially filled with pure SO3. After a period of time, the following equilibrium is…

A: Predicting the extent of reaction. The magnitude of the equilibrium constant gives an idea relative…

Q: b. H2(g) + CO2(g) → H20(g) + CO(g) AH = +9.9 kcal Shift (рнг) (рсоэ) (рнго) (рсо) K Removal of H2…

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Question

9. Gaseous sulfur dioxide reacts with oxygen to from gaseous sulfur trioxide.
a. Write a balanced chemical equation for this reaction.
b. At some temperature, the equilibrium constant for this reaction is 16. If 1.0 mole of sulfur dioxide, 1.8
mole of oxygen, and 4.0 mole of sulfur trioxide are placed in a 2.0 L flask at this temperature will the
reaction proceed to the products or to the reactants?
c. Compare the amount of reactants and products at equilibrium to the amount of reactants and products
added to the flask in part b.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Chapter 1 question 6: Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 50.0L tank with 4.6 mol of ammonia gas and 4.5 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.2 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.
If we represent the equilibrium as: 2 NO2(g) = N204(g) We can conclude that: |1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of NO2: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
2. Consider the following equilibrium. Which way will the system shift, if at all? How would the following changes affect the partial pressures of each gas at the new equilibrium, if at all? How will the equilibrium constant change, if at all?
For the equilibrium reaction: 2 NOCl(g) 2 NO(g) + Cl2(g)5.00 mol NOCl was placed in an otherwise empty 1.00-L flask at a certain temperature. When the system reaches equilibrium 0.83 mol NO is present. Calculate Kcat that temperature. A. 1.6×10-2 B. 61 C. 3.3×10-2 D. 1.1×10-2
Given each equilibrium constant, state whether the reactants are favored, the products are favored, or both the reactants and products are present at equilibrium. a. 5.0 × 10 −4 b. 4.4 × 10 5 c. 350 d. 0.35
In the ideal gas experiment, the students forgot to record the equilibrium temperature after reacting the magnesium ribbon to the acid. For their calculations, they assumed this temperature to be 25 °C. If the actual temperature was 28 °C, how will this affect the value of the calculated moles of gas produced? Will it increase or decrease?
c. HF & HCIO4 d. HBr & LIOH e. CH3COOH & KOH A sealed 1.00L flask is charged with 0.500 mol of I, and 0.500 mol of Br2. An equilibrium reaction ensues: 12 (g) + Br2 (g) =2 IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of K is Select one: O a. K= 6.10 O b. K = 2.82 OC K = 882 Od. K= 110 Oe K= 131 en 13 The heat capacity of silver (Ag. 107.9 g maol), is 0.232 J g'K Calculate the energy needed to heat 2e mo saved II
Chamber A contains 40% oxygen and Chamber B contains 20% oxygen. Chambers are connected by a tube and the oxygen molecules are free to cross. Which of the following is most likely to occur over time? A. all of the oxygen will move into chamber B B. The oxygen concentration will remain the same of both sides C. Some oxygen will move chamber A to chamber B until equilibrium reached D. Some oxygen will move chamber B to chamber A until one side has more oxygen
Use Le Châtelier’s Principle to explain the effect each of the following changes will have upon the system—will the equilibrium shift toward the product or reactant side? Why? N2(g) + 3 H2(g) ↔ 2 NH3(g) + heat a. If more hydrogen is added to the system the equilibrium will shift to the..... (pick one and explain)i. Right ii. Left iii. Remains unchanged b. If ammonia is removed from the system the equilibrium will shift to the..... (pick one and explain)i. Right ii. Left iii. Remains unchanged c. If nitrogen is removed from the system the equilibrium will shift to the..... (pick one and explain)
If the equilibrium constant, K, is greater than 1 which of the following is true? Select one: a. There are more products than reactants. b. There are more reactants than products. O c. We have all reactants and zero products. O d. The number of reactants equals the number of products.
13. H.(g)+F(g) = 2HF(g) At this temperature, 0.481 Kc =9.41 x 10³ mol H₂ and 0.481 mol F₂ were placed in a 0.750 L container to react. What concentration of HF is present at equilibrium? a. 0.588 M b. 0.600 M c. 1.18 M d. 1.20 M #431 10 e. 1.79 M السلام امن mla