Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Question
Is two right ? And need help With three. Need to write the equilibrium and equation
![The Ka of nitrous acid.
HNO2 caq)
+ H20e) NO 2 (aq) + Hgơc42)
ka: IHS0] [NO]
T HNO,]
2. The Kp of ammonia.
NHsan) + H20 = NHy + OH-
TOH-3 [NH]
kB =
[NHs]
3. The Ka and Kb for bicarbonate.
NaHCOs +
4. The Kp for sulfate.
5. The Ka for CH3NH3*.
for CH-NH.](https://content.bartleby.com/qna-images/question/560885b1-95a6-46a1-8479-9132da42c8bd/84a4a321-aba3-4220-91c3-eccc5055fd08/aqkyhor_processed.jpeg)
Transcribed Image Text:The Ka of nitrous acid.
HNO2 caq)
+ H20e) NO 2 (aq) + Hgơc42)
ka: IHS0] [NO]
T HNO,]
2. The Kp of ammonia.
NHsan) + H20 = NHy + OH-
TOH-3 [NH]
kB =
[NHs]
3. The Ka and Kb for bicarbonate.
NaHCOs +
4. The Kp for sulfate.
5. The Ka for CH3NH3*.
for CH-NH.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by stepSolved in 2 steps with 2 images
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
- Decide whether each of the following statements is true or false. If false, change the wording of the statement to make it true. a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction. d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.arrow_forwardThanks please anwser the question properly thanks ?arrow_forward2. 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?arrow_forward
- Refer to the following equation and data and answer question. CO (g) + 3H2 (g) CH4 (g) + H2O (g) (Note: all species are in gas phase) At a certain temperature, 0.100 mole CO and 0.300 mole H2 are placed in a 1.00 L vessel . After the reaction has reached equilibrium, the vessel contains 0.0387 mol H2O. How much CO is there at equilibrium? Hint: you have been given an equilibrium concentration, you can use it to find x and equilibrium concentrations of other species. 3.29 M 0.209 M 3.41 x 10 -4 M 1.43 x 10 -1 M 6.93 x 10-2 M 0.103 M 0.0613 M 2.60 x 10 -3 Marrow_forward2. 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?arrow_forwardWhile ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene with water vapor at elevated temperatures. (CH,CH,) A chemical engineer studying this reaction fills a 75.0 L tank with 5.0 mol of ethylene gas and 20. mol of water vapor. When the equilibrium she determines that it contains 1.1 mol of ethylene gas and 16.1 mol of water vapor. mixture has come to The engineer then adds another 1.7 mol of ethylene, and allows the reached the second time. Round your answer to 2 significant digits. mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is I molarrow_forward
- 10. Initially a 1.0 L vessel contains 10.0 mol of NO and 6.0 mol of O2 at a certain temperature. 2 NO (g) + O2 (g) = 2 NO2 (g)arrow_forwardTwo gaseous molecules react and produce two other gases molecules in an equilibrium reaction. What happens when the pressure is decreased? A  it shifts to the right B  more products form C It shifts to the left D Nothing happensarrow_forwardMost medications have an expiration date. Describe with respect to equilibrium, what occurring as the medication ages. Is there any of the medication left after the expiration date?arrow_forward
- In a system at equilibrium, it is true that a. the rate of the forward reaction exceeds that of the reverse b. the rate of the forward reaction is lower than that of the reverse reaction c. the rate of the forward reaction is equal to the rate of the reverse reaction d. more than one response is correctarrow_forwardAt constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increas of moles of gas in the system.arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY