Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 12, Problem 24QAP
Consider the decomposition at 25°C of one mole of NOBr gas into NO and Br2 gases. At equilibrium, the concentrations of NOBr, NO, and Br2 gases are 0.0162 M, 0.0011 M, and 0.072 M, respectively.
(a) Write a balanced equation for the reaction.
(b) Calculate K for the reaction at 25°C. (Note that the gases need to be expressed as pressure in atm.)
Expert Solution & Answer
Trending nowThis is a popular solution!
Chapter 12 Solutions
Chemistry: Principles and Reactions
Ch. 12 - The following data are for the system A(g)2B(g)...Ch. 12 - The following data are for the system A(g)2B(g)...Ch. 12 - Prob. 3QAPCh. 12 - Complete the table below for the reaction...Ch. 12 - Write the equilibrium expressions (K) for the...Ch. 12 - Write the equilibrium expressions (K) for the...Ch. 12 - Write the equilibrium expressions (K) for the...Ch. 12 - Write the equilibrium expressions (K) for the...Ch. 12 - Given the following descriptions of reversible...Ch. 12 - Given the following descriptions of reversible...
Ch. 12 - Write an equation for an equilibrium system that...Ch. 12 - Write a chemical equation for an equilibrium...Ch. 12 - Consider the following reaction at 250C:...Ch. 12 - Consider the following reaction at 1000 C:...Ch. 12 - At 627C, K=0.76 for the reaction...Ch. 12 - At 800C, K=2.2104 for the following reaction...Ch. 12 - Prob. 17QAPCh. 12 - Given the following data at 25C...Ch. 12 - Given the following data at a certain temperature,...Ch. 12 - Consider the following hypothetical reactions and...Ch. 12 - When one mole of carbon disulfide gas reacts with...Ch. 12 - Calculate K for the formation of methyl alcohol at...Ch. 12 - Ammonium carbamate solid (NH4CO2NH2) decomposes at...Ch. 12 - Consider the decomposition at 25C of one mole of...Ch. 12 - Consider the decomposition of ammonium hydrogen...Ch. 12 - A sealed flask has 0.541 atm of SO3 at 1000 K. The...Ch. 12 - A gaseous reaction mixture contains 0.30 atm SO2,...Ch. 12 - For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at...Ch. 12 - The reversible reaction between hydrogen chloride...Ch. 12 - The reversible reaction between hydrogen chloride...Ch. 12 - A compound, X, decomposes at 131C according to the...Ch. 12 - Consider the following reaction at 75C:...Ch. 12 - Consider the reaction between nitrogen and steam:...Ch. 12 - At 500C, k for the for the formation of ammonia...Ch. 12 - At a certain temperature, K is 4.9 for the...Ch. 12 - At a certain temperature, K=0.29 for the...Ch. 12 - For the reaction N2(g)+2H2O(g)2NO(g)+2H2(g) K is...Ch. 12 - Nitrogen dioxide can decompose to nitrogen oxide...Ch. 12 - Consider the following reaction:...Ch. 12 - Consider the hypothetical reaction at 325C...Ch. 12 - At a certain temperature, the equilibrium constant...Ch. 12 - At 460C, the reaction SO2(g)+NO2(g)NO(g)+SO3(g)...Ch. 12 - Solid ammonium iodide decomposes to ammonia and...Ch. 12 - Consider the following decomposition at 80C....Ch. 12 - Hydrogen cyanide, a highly toxic gas, can...Ch. 12 - At 800 K, hydrogen iodide can decompose into...Ch. 12 - For the following reactions, predict whether the...Ch. 12 - Follow the directions of Question 47 for the...Ch. 12 - Consider the system SO3(g)SO2(g)+12 O2(g)H=98.9kJ...Ch. 12 - Consider the system...Ch. 12 - Predict the direction in which each of the...Ch. 12 - Predict the direction in which each of the...Ch. 12 - At a certain temperature, nitrogen and oxygen...Ch. 12 - Consider the following hypothetical reaction:...Ch. 12 - Iodine chloride decomposes at high temperatures to...Ch. 12 - Sulfur oxychloride, SO2Cl2, decomposes to sulfur...Ch. 12 - For the following reaction C(s)+2H2(g)CH4(g)...Ch. 12 - For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627....Ch. 12 - For a certain reaction, H is +33 kJ. What is the...Ch. 12 - Prob. 60QAPCh. 12 - Hemoglobin (Hb) binds to both oxygen and carbon...Ch. 12 - Mustard gas, used in chemical warfare in World War...Ch. 12 - Prob. 63QAPCh. 12 - For the decomposition of CaCO3 at 900C, K=1.04....Ch. 12 - Isopropyl alcohol is the main ingredient in...Ch. 12 - Consider the equilibrium H2(g)+S(s)H2S(g)When this...Ch. 12 - Prob. 67QAPCh. 12 - The following data apply to the unbalanced...Ch. 12 - Consider the reaction: A(g)+2B(g)+C(s)2D(g)At 25C,...Ch. 12 - For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273...Ch. 12 - Consider the system A(g)+2B(g)+C(g)2D(g)at 25C. At...Ch. 12 - The graph below is similar to that of Figure 12.2....Ch. 12 - Prob. 73QAPCh. 12 - The figures below represent the following reaction...Ch. 12 - Prob. 75QAPCh. 12 - Prob. 76QAPCh. 12 - Consider the following reaction at a certain...Ch. 12 - Prob. 78QAPCh. 12 - Ammonia can decompose into its constituent...Ch. 12 - Hydrogen iodide gas decomposes to hydrogen gas and...Ch. 12 - For the system SO3(g)SO2(g)+12 O2(g)at 1000 K,...Ch. 12 - A student studies the equilibrium I2(g)2I(g)at a...Ch. 12 - At a certain temperature, the reaction...Ch. 12 - Benzaldehyde, a flavoring agent, is obtained by...Ch. 12 - Prob. 85QAPCh. 12 - Prob. 86QAP
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
- At 500C, k for the for the formation of ammonia from nitrogen and hydrogen gases is 1.5105. N2(g)+3H2(g)2NH3(g)Calculate the equilibrium partial pressure of hydrogen if the equilibrium partial pressures of ammonia and nitrogen are 0.015 atm and 1.2 atm, respectively.arrow_forwardYou place 0.600 mol of nitrogen, N2, and 1.800 mol of hydrogen, H2, into a reaction vessel at 450C and 10.0 atm. The reaction is N2(g)+3H2(g)2NH3(g) What is the composition of the equilibrium mixture if you obtain 0.048 mol of ammonia, NH3, from it?arrow_forwardConsider the following hypothetical reaction: X2(g)+R(s)X2R(g) R has a molar mass of 73 g/mol. When equilibrium is established, a 2.5-L reaction vessel at 125C contains 15.0 g of R, 4.3 atm of X2, and 0.98 atm of X2R. (a) Calculate K for the reaction at 125C. (b) The mass of R is doubled. What are the partial pressures of X2 and X2R when equilibrium is reestablished? (c) The partial pressure of X2 is decreased to 2.0 atm. What are the partial pressures of X2 and X2R when equilibrium is reestablished?arrow_forward
- Given these data at a certain temperature, 2H2(g)+O2(g)2H2O(g)Kc=3.21081N2(g)+3H2(g)2NH3(g)Kc=3.5108 calculate Kc for the reaction of ammonia with oxygen to give N2(g) and H2O(g).arrow_forwardAt a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?arrow_forwardA 2.500-mol sample of phosphorus pentachloride, PCl5, decomposes at 160C and 1.00 atm to give 0.338 mol of phosphorus trichloride, PCl3, at equilibrium. PCl5(g)PCl3(g)+Cl2(g) What is the composition of the final reaction mixture?arrow_forward
- Methanol, a common laboratory solvent, poses a threat of blindness or death if consumed in sufficient amounts. Once in the body, the substance is oxidized to produce formaldehyde (embalming fluid) and eventually formic acid. Both of these substances are also toxic in varying levels. The equilibrium between methanol and formaldehyde can be described as follows: CH3OH(aq)H2CO(aq)+H2(aq) Assuming the value of K for this reaction is 3.7 1010, what are the equilibrium concentrations of each species if you start with a 1.24 M solution of methanol? What will happen to the concentration of methanol as the formaldehyde is further converted to formic acid?arrow_forward. Gaseous phosphorus pentachloride decomposes according to the reaction PCl5(g)PCl3(g)+Cl2(g)The equilibrium system was analyzed at a particular temperature, and the concentrations of the substances present were determined to be [PCl5]=1.1102M,[PCl3]=0.325M. and [Cl2]=3.9103M. Calculate the value of K for the reaction.arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781285199030Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781285199030
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemical Equilibria and Reaction Quotients; Author: Professor Dave Explains;https://www.youtube.com/watch?v=1GiZzCzmO5Q;License: Standard YouTube License, CC-BY