the equilibrium pressure of Bf2(8) 15.54 At 218 °C, K̟ = 1.2 × 10-4 for the equilibrium NH4SH(s) = NH3(g) + H2S(g) Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH SH is placed in a closed vessel at 218 °C and decomposes until equilibrium is reached. 15.55 Consider the reaction CaSO4(s) = Ca2+(aq) + SO,² (aq) At 25 °C, the equilibrium constant is K, = 2.4 × 10¯³ for this reaction. (a) If excess CASO.(s) is mixed with water at 25 °C to produce a saturated solution of CaSO4, what are the equilibrium concentrations of Ca²+ and SO7? (b) If the resulting solution has a volume of 1.4 L, what is the minimum mass of CASO.(s) needed to achieve equilibrium? 4. 15.56 At 80 °C, K̟ = 1.87 × 10-3 for the reaction %3D PH3BCI3(s) = PH3(g) + BC13(g) (a) Calculate the equilibrium concentrations of PH3 and BCI3 if a solid sample of PH3BC13 is placed in a closed ves- sel at 80 °C and decomposes until equilibrium is reached. (b) If the flask has a volume of 0.250 L, what is the mini- mum mass of PH3BC13(s) that must be added to the flask to achieve equilibrium? 15.57 For the reaction I2(g) + Br2(g) 2 IBr(g), K. = 280 at 150 °C. Suppose that 0.500 mol IBr in a 2.00-L flask is allowed to reach equilibrium at 150°C. What are the equilibrium concentrations of IBr, I2, and Br,? 15.58 At 25 °C, the reaction CaCrO4(s) Ca2 (aq)+ CrO2 (aq) has an equilibrium constant K = 7.1 × 10-4. What are the equilibrium concentrations of Ca?+ saturated solution of CaCrO4? %3D oo and CrO,2- in a 4 15.59 Methane, CH4, reacts with I, according to the reactio
the equilibrium pressure of Bf2(8) 15.54 At 218 °C, K̟ = 1.2 × 10-4 for the equilibrium NH4SH(s) = NH3(g) + H2S(g) Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH SH is placed in a closed vessel at 218 °C and decomposes until equilibrium is reached. 15.55 Consider the reaction CaSO4(s) = Ca2+(aq) + SO,² (aq) At 25 °C, the equilibrium constant is K, = 2.4 × 10¯³ for this reaction. (a) If excess CASO.(s) is mixed with water at 25 °C to produce a saturated solution of CaSO4, what are the equilibrium concentrations of Ca²+ and SO7? (b) If the resulting solution has a volume of 1.4 L, what is the minimum mass of CASO.(s) needed to achieve equilibrium? 4. 15.56 At 80 °C, K̟ = 1.87 × 10-3 for the reaction %3D PH3BCI3(s) = PH3(g) + BC13(g) (a) Calculate the equilibrium concentrations of PH3 and BCI3 if a solid sample of PH3BC13 is placed in a closed ves- sel at 80 °C and decomposes until equilibrium is reached. (b) If the flask has a volume of 0.250 L, what is the mini- mum mass of PH3BC13(s) that must be added to the flask to achieve equilibrium? 15.57 For the reaction I2(g) + Br2(g) 2 IBr(g), K. = 280 at 150 °C. Suppose that 0.500 mol IBr in a 2.00-L flask is allowed to reach equilibrium at 150°C. What are the equilibrium concentrations of IBr, I2, and Br,? 15.58 At 25 °C, the reaction CaCrO4(s) Ca2 (aq)+ CrO2 (aq) has an equilibrium constant K = 7.1 × 10-4. What are the equilibrium concentrations of Ca?+ saturated solution of CaCrO4? %3D oo and CrO,2- in a 4 15.59 Methane, CH4, reacts with I, according to the reactio
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...
Related questions
Concept explainers
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question
Question 15.56 part A only
Transcribed Image Text:the equilibrium pressure of Bf2(8)
15.54 At 218 °C, K̟ = 1.2 × 10-4 for the equilibrium
NH4SH(s) = NH3(g) + H2S(g)
Calculate the equilibrium concentrations of NH3 and H2S
if a sample of solid NH SH is placed in a closed vessel at
218 °C and decomposes until equilibrium is reached.
15.55 Consider the reaction
CaSO4(s) = Ca2+(aq) + SO,² (aq)
At 25 °C, the equilibrium constant is K, = 2.4 × 10¯³ for
this reaction. (a) If excess CASO.(s) is mixed with water
at 25 °C to produce a saturated solution of CaSO4, what
are the equilibrium concentrations of Ca²+ and SO7?
(b) If the resulting solution has a volume of 1.4 L, what
is the minimum mass of CASO.(s) needed to achieve
equilibrium?
4.
15.56 At 80 °C, K̟ = 1.87 × 10-3 for the reaction
%3D
PH3BCI3(s) = PH3(g) + BC13(g)
(a) Calculate the equilibrium concentrations of PH3 and
BCI3 if a solid sample of PH3BC13 is placed in a closed ves-
sel at 80 °C and decomposes until equilibrium is reached.
(b) If the flask has a volume of 0.250 L, what is the mini-
mum mass of PH3BC13(s) that must be added to the flask
to achieve equilibrium?
15.57 For the reaction I2(g) + Br2(g)
2 IBr(g), K. = 280
at 150 °C. Suppose that 0.500 mol IBr in a 2.00-L flask
is allowed to reach equilibrium at 150°C. What are the
equilibrium concentrations of IBr, I2, and Br,?
15.58 At 25 °C, the reaction
CaCrO4(s) Ca2
(aq)+ CrO2 (aq)
has an equilibrium constant K = 7.1 × 10-4. What are
the equilibrium concentrations of Ca?+
saturated solution of CaCrO4?
%3D
oo
and CrO,2- in a
4
15.59 Methane, CH4, reacts with I, according to the reactio
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!
Trending now
This is a popular solution!
Step by step
Solved 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.Recommended textbooks for you
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
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