Chemistry: Atoms First
18th Edition
ISBN: 9781938168154
Author: Richard Langley, Klaus Theopold, Paul Flowers
Publisher: OpenStax College
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Textbook Question
Chapter 13, Problem 5E
If the concentrations of products and reactants are equal, is the system at equilibrium?
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Students have asked these similar questions
Using reaction free energy to predict equilibrium composition
Consider the following equilibrium:
2NOCI (g) 2NO (g) + Cl2 (g) AGº =41. kJ
Now suppose a reaction vessel is filled with 4.50 atm of nitrosyl chloride (NOCI) and 6.38 atm of chlorine (C12) at 212. °C. Answer the following questions
about this system:
?
rise
Under these conditions, will the pressure of NOCI tend to rise or fall?
x10
fall
Is it possible to reverse this tendency by adding NO?
In other words, if you said the pressure of NOCI will tend to rise, can that
be changed to a tendency to fall by adding NO? Similarly, if you said the
pressure of NOCI will tend to fall, can that be changed to a tendency to
rise by adding NO?
yes
no
If you said the tendency can be reversed in the second question, calculate
the minimum pressure of NO needed to reverse it.
Round your answer to 2 significant digits.
0.035 atm
✓
G
00.
18
Ar
Highlight each glycosidic bond in the molecule below. Then answer the questions in the table under the drawing area.
HO-
HO-
-0
OH
OH
HO
NG
HO-
HO-
OH
OH
OH
OH
NG
OH
€
+
Suppose the molecule in the drawing area below were reacted with H₂ over a platinum catalyst. Edit the molecule to show what would happen to it. That is, turn
it into the product of the reaction.
Also, write the name of the product molecule under the drawing area.
Name: ☐
H
C=0
X
H-
OH
HO-
H
HO-
-H
CH₂OH
×
Chapter 13 Solutions
Chemistry: Atoms First
Ch. 13 - What does it mean to describe a reaction as...Ch. 13 - When writing an equation, how is a reversible...Ch. 13 - If a reaction is reversible, when can it be said...Ch. 13 - Is a system at equilibrium if the rate constants...Ch. 13 - If the concentrations of products and reactants...Ch. 13 - Explain why there may be an infinite number of...Ch. 13 - Explain why an equilibrium between Br2(l)andBr2(g)...Ch. 13 - If you observe the following reaction at...Ch. 13 - Among the solubility rules previously discussed is...Ch. 13 - Among the solubility rules previously discussed is...
Ch. 13 - Benzene is one of the compounds used as octane...Ch. 13 - Show that the complete chemical equation, the...Ch. 13 - For a titration to be effective, the reaction must...Ch. 13 - For a precipitation reaction to be useful in a...Ch. 13 - Write the mathematical expression for the reaction...Ch. 13 - Write the mathematical expression for the reaction...Ch. 13 - The initial concentrations or pressures of...Ch. 13 - The initial concentrations or pressures of...Ch. 13 - The following reaction has KP=4.5010-5at720K ....Ch. 13 - Determine if the following system is at...Ch. 13 - Which of the systems described in Exercise 13.15...Ch. 13 - Which of the systems described in Exercise 13.16...Ch. 13 - For which of the reactions in Exercise 13.15 does...Ch. 13 - For which of the reactions in Exercise 13.16 does...Ch. 13 - Convert the values of KC to values of KP to the...Ch. 13 - Covert the values of Kc to the values of KP or the...Ch. 13 - What is the value of the equilibrium constant...Ch. 13 - Write the expression of the reaction quotient for...Ch. 13 - Write the reaction quotient expression for the...Ch. 13 - What is the approximate value of the equilibrium...Ch. 13 - The following equation represents a reversible...Ch. 13 - Explain how to recognize the conditions under...Ch. 13 - What property of a reaction can we use to predict...Ch. 13 - The following reaction occurs when a burner on a...Ch. 13 - A necessary step in the manufacture of sulfuric...Ch. 13 - Suggest four ways in which the concentration of...Ch. 13 - Suggest four ways in which the concentration of...Ch. 13 - How will an increase in temperature affect each of...Ch. 13 - How will an increase in temperature affect each of...Ch. 13 - Methanol can be prepared from carbon monoxide and...Ch. 13 - Nitrogen and oxygen react at high temperatures....Ch. 13 - Water gas, a mixture of H2 and CO, is an important...Ch. 13 - Pure iron metal can be produced by the reduction...Ch. 13 - Ammonia is a weak base that reacts with water...Ch. 13 - Acetic acid is a weak acid that reacts with water...Ch. 13 - Suggest two ways in which the equilibrium...Ch. 13 - How can the pressure of water vapor be increased...Ch. 13 - A solution is saturated with silver sulfate and...Ch. 13 - The amino acid alanine has two isomers, -alanine...Ch. 13 - A reaction is represented by this equation:...Ch. 13 - A reaction is represented by this equation:...Ch. 13 - What is the value of the equilibrium constant at...Ch. 13 - Hydrogen is prepared commercially by the reaction...Ch. 13 - A 0.72-m01 sample of PCl5 is put into a 1.00-L...Ch. 13 - At 1 atm and 25 C, NO2 with an initial...Ch. 13 - Calculate the value of the equilibrium constant Kp...Ch. 13 - When heated, iodine vapor dissociates according to...Ch. 13 - A sample of ammonium chloride was heated in a...Ch. 13 - At a temperature of 60 C, the vapor pressure of...Ch. 13 - Complete the changes in concentrations (or...Ch. 13 - Complete the changes in concentrations (or...Ch. 13 - Why are there no changes specified for Ni in...Ch. 13 - Why are there no changes specified for NH4HS in...Ch. 13 - Analysis of the gases in a sealed reaction vessel...Ch. 13 - Calculate the number of moles of HI that are at...Ch. 13 - What is the pressure of BrCl in an equilibrium...Ch. 13 - What is the pressure of CO2 in a mixture at...Ch. 13 - Cobalt metal can be prepared by reducing cobalt...Ch. 13 - Carbon reactswith water vapor at elevated...Ch. 13 - Sodium sulfate 10-hydrate, Na2SO410H2O, dehydrates...Ch. 13 - Calcium chloride 6-hydrate, CaC12.6H2O, dehydrates...Ch. 13 - A student solved the following problem and found...Ch. 13 - A student solved the following problem and found...Ch. 13 - Assume that the change in concentration of N2O4 is...Ch. 13 - Assume that the change in concentration of COC12...Ch. 13 - Assume that the change in pressure of H2S is small...Ch. 13 - What are all concentrations after a mixture that...Ch. 13 - Calculate the number of grams of HI that are at...Ch. 13 - Butane exists as two isomers, n -butane and...Ch. 13 - What is the minimum mass of CaCO3 required to...Ch. 13 - The equilibrium constant (Kc) for this reaction is...Ch. 13 - In a 3.0-L vessel, the following equilibrium...Ch. 13 - The equilibrium constant (Kc) for this reaction is...Ch. 13 - Antimony pentachloride decomposes according to...Ch. 13 - Consider the equilibrium...Ch. 13 - The binding of oxygen by hemoglobin (Hb), giving...Ch. 13 - Liquid N2o3 is dark blue at low temperatures, but...Ch. 13 - A 1.00-L vessel at 400C contains the following...Ch. 13 - Calculate the equilibrium constant at 25 C for...Ch. 13 - Calculate the equilibrium constant at the...Ch. 13 - Calculate the equilibrium constant at the...Ch. 13 - Consider the following reaction at 298 K:...Ch. 13 - Determine the normal boiling point (inkelvin) of...Ch. 13 - Under what conditions is N2O3(g)NO(g)+NO2(g)...Ch. 13 - At room temperature, the equilibrium constant (Kw)...Ch. 13 - Hydrogen sulfide is a pollutant found in natural...Ch. 13 - Consider the decomposition of CaCO3(s) into...Ch. 13 - In the laboratory, hydrogen chloride (HCl(g)) and...Ch. 13 - Benzene can be prepared from acetylene....Ch. 13 - Carbon dioxide decomposes into CO and O2 at...Ch. 13 - Carbon tetrachloride, an important industrial...Ch. 13 - Acetic acid, CH3CO2H, Can form a dimer,...
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