**Sulfur dioxide and nitrogen dioxide react at 298 K via the reaction:**\[ \text{SO}_2(\text{g}) + \text{NO}_2(\text{g}) \leftrightarrow \text{SO}_3(\text{g}) + \text{NO}(\text{g}) \]A system at equilibrium contains 0.394 mol SO₂, 0.394 mol NO₂, 0.812 mol SO₃, and 0.660 mol NO. O₂ is added to the container and NO reacts completely with the O₂. Calculate the amount of SO₃ in the container after the system returns to equilibrium.**mass SO₃:**\[ \boxed{\hspace{3cm}} \, \text{g} \]

For any reaction, the Equilibrium constant is defined as the ratio of the concentration of product…

Sulfur dioxide and nitrogen dioxide react at 298 K via the reaction SO₂(g) + NO₂(g) = SO3(g) + NO(g) A system at equilibrium contains 0.394 mol SO₂, 0.394 mol NO₂, 0.812 mol SO3, and 0.660 mol NO. O₂ is added to the container and NO reacts completely with the O₂. Calculate the amount of SO3 in the container after the system returns to equilibrium. g mass SO3:

Sulfur dioxide and nitrogen dioxide react at 298 K via the reaction SO₂(g) + NO₂(g) = SO3(g) + NO(g) A system at equilibrium contains 0.394 mol SO₂, 0.394 mol NO₂, 0.812 mol SO3, and 0.660 mol NO. O₂ is added to the container and NO reacts completely with the O₂. Calculate the amount of SO3 in the container after the system returns to equilibrium. g mass SO3:

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 69QRT

See similar textbooks

Similar questions

Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25C
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.
A process that is reactant-favored at equilibrium can never be spontaneous. This statement is (a) true (b) false
The equilibrium constant for a reaction decreases as temperature increases. Explain how this observation is used to determine the sign of either H or S.
Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.
If wet silver carbonate is dried in a stream of hot air. the air must have a certain concentration level of carbon dioxide to prevent silver carbonate from decomposing by the reaction Ag2CO3(s)Ag2O(s)+CO2(g) H for this reaction is 79.14 kJ/mol in the temperature range of 25 to 125C. Given that the partial pressure of carbon dioxide in equilibrium with pure solid silver carbonate is 6.23 103 torr at 25C, calculate the partial pressure of CO2 necessary to prevent decomposition ofAg2CO3 at 110C. (Hint: Manipulate the equation in Exercise 79.)
Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Methanol can be synthesized by means of the equilibriumreaction CO(g)+2H2(g)CH3OH(g) for which the equilibrium constant at 225°C is 6.08103. Assume that the ratio of the pressures of CO(g) and H2(g) is 1:2. What values should they have if the partial pressureof methanol is to be 0.500 atm?
Given the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.