(a)
Interpretation:
The value of equilibrium constant
Concept Introduction:
In an equilibrium constant expression, the powers of the chemical species help in predicting the
(b)
Interpretation:
Whether the reaction,
Concept Introduction:
To predict whether a reaction is endothermic or exothermic, find out the change in enthalpy of the reaction which is obtained by subtracting the activation energy of the backward reaction from the forward reaction. If the enthalpy change is positive, it is an endothermic reaction and if it is negative then it is an exothermic reaction
(c)
Interpretation:
The effect of raising the temperature on the rate constants and equilibrium constant of the reaction has to be predicted.
Concept Introduction:
A reaction is said to be in equilibrium if the rate at which the forward reaction takes place becomes equal to the rate at which the backward reaction takes place. If any of the factors that affect the equilibrium changes, then the reaction shifts in either forward or backward direction so that the equilibrium condition is reestablished.
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Chapter 7 Solutions
ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM
- Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.arrow_forwardAt 1 atm and 25 C, NO2 with an initial concentration of 1.00 M is 3.3103 decomposed into NO and O2. Calculate the value of the equilibrium constant for the reaction. 2NO2(g)2NO(g)+O2(g)arrow_forwardWhich reaction mechanism assumptions are unimportant in describing simple ionic reactions between cations and anions? Why?arrow_forward
- Silicon forms a series of compounds analogous to the al-kanes and having the general formula SinH2n+2. The first of these compounds is silane, SiH4, which is used in the electronics industry to produce thin ultrapure silicon films. SiH4(g) is somewhat difficult to work with because it is py-ropboric at room temperature—meaning that it bursts into flame spontaneously when exposed to air. (a) Write an equation for the combustion of SiH4(g). (The reaction is analogous to hydrocarbon combustion, and SiO2 is a solid under standard conditions. Assume the water produced will be a gas.) (b) Use the data from Appendix E to calculate ? for this reaction. (c) Calculate G and show that the reaction is spontaneous at 25°C. (d) Compare G for this reaction to the combustion of methane. (See the previous problem.) Are the reactions in these two exercises enthalpy or entropy driven? Explain.arrow_forward7-17 If a certain reaction takes 16 h to go to completion at 10°C, what temperature should we run it if we want it to go to completion in 1 h?arrow_forward7-22 If you add a piece of marble, CaCO3 to a 6 M HCI solution at room temperature, you will see some bubbles form around the marble as gas slowly rises. If you crush another piece of marble and add it to the same solution at the same temperature, you will see vigorous gas formation, so much so that the solution appears to be boiling. Explain.arrow_forward
- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forward(a) If Qc 7 Kc, how must the reaction proceed to reachequilibrium? (b) At the start of a certain reaction, onlyreactants are present; no products have been formed.What is the value of Qc at this point in the reaction?arrow_forwardThe equilibrium constant, Kc , for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) is 6.90 x 103 . (a) What is Kc for the reaction 2 SO3 (g) → 2 SO2 (g) + O2 (g) (b) What is Kc for the reaction SO2 (g) + 1/2 O2 (g) → SO3 (g)arrow_forward
- At 25 ∘C25 ∘C, the equilibrium partial pressures for the reaction 3A(g)+3B(g)↽−−⇀C(g)+3D(g)3A(g)+3B(g)↽−−⇀C(g)+3D(g) were found to be ?A=4.38PA=4.38 atm, ?B=4.26PB=4.26 atm, ?C=4.32PC=4.32 atm, and ?D=4.83PD=4.83 atm. What is the standard change in Gibbs free energy of this reaction at 25 ∘C25 ∘C?arrow_forwardThe equilibrium system 2SO2(g)+ O2(g) = 2S03(g) is an exothermic reaction. Which change will result in an increase in the concentration of SO3 when equilibrium is re-established? (A) a decrease in pressure (B) the removal of SO2(g) (C) an increase in temperature (D) a decrease in volume of the containerarrow_forwardThe equilibrium constant for the reaction, I2(s) + Br2(g) ⇋ 2 IBr(g) is 0.25 at 25 °C. (a) Calculate ΔrG⦵ for this reaction. (b) Bromine gas is introduced into a container with excess solid iodine. The pressure and temperature are held at 0.25 atm and 25 °C, respectively. Find the partial pressure of IBr(g) at equilibrium. Assume that the bromine is in the liquid form and that the vapour pressure of iodine is negligible. (c) In fact, solid iodine has a measurable vapour pressure at 25 °C. In this case, how would the calculation have to be modified?arrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
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