*00FL山Rttps://WWW-awu.aleks.com/alekscgi/x/lsl.exe/1o_u-lgNslkr7j8P3jH-IQUHIQg6bJxmeSyVpHOEB1plef9xyC5Ca9QldFNDUsAt... AO ADVANCED GENERAL CHEMISTRY0/5Calculating an equilibrium constant from an equilibrium.Hydrogen bromide and oxygen react to form bromine and water, like this:4 HBr(g) + O,(g) → 2 Br,(g) + 2 H,0(g)Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen bromide, oxygen, bromine, and water has the following composition:compound pressure at equilibriumHBr76.6 atm79.4 atmBr27.76 atm5.82 atmo'HCalculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.ExplanationCheckO2022 McGraw Hill LLC. AllRights Reserved. Terms of Use Privacy Center Accessibility9:373/18/2DECF5F8r pgDn.OLF12PrtScrInsertDeleteLLPgUp24BackspaceLock{[Enter4ShiftAltAltCtrl

rogen bromide and oxygen react to form bromine and water, like this: 4 HBr(g) + O,(9) → 2 Br,(9) + 2 H,O(g) 50, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen bromide, oxygen, bromine, and water compound pressure at equilibrium HBr 76.6 atm 02 79.4 atm Br2 7.76 atm H,O 5.82 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. - 0 K = Explanation Check 2022 McG

rogen bromide and oxygen react to form bromine and water, like this: 4 HBr(g) + O,(9) → 2 Br,(9) + 2 H,O(g) 50, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen bromide, oxygen, bromine, and water compound pressure at equilibrium HBr 76.6 atm 02 79.4 atm Br2 7.76 atm H,O 5.82 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. - 0 K = Explanation Check 2022 McG

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 27P

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Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?
Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
The equilibrium between nitrogen monoxide, oxygen, and nitrogen dioxide may be expressed in the equation 2NO(g)+O2(g)2NO(g). Write the equilibrium constant expression for this equation. Then express the same equilibrium in at least two other ways, and write the equilibrium constant expression for each. Are the constants numerically equal? Cite some evidence to support your answer. Nitrogen monoxide and oxygen, both colorless gases, react to form reddish-brown nitrogen dioxide.