Kinetics Add your explanation there Given the reaction 2 Cl2 (g) + 2H₂O(g) → 4HCl (g) O2(g), AHO chemical reaction = -742 kJ/mol + Determine the direction in which the equilibrium will be shifted by increasing the concentration of Cl₂ in the reaction Ob) shifts to right Oc) no change Oa) shifts to left

Kinetics Add your explanation there Given the reaction 2 Cl2 (g) + 2H₂O(g) → 4HCl (g) O2(g), AHO chemical reaction = -742 kJ/mol + Determine the direction in which the equilibrium will be shifted by increasing the concentration of Cl₂ in the reaction Ob) shifts to right Oc) no change Oa) shifts to left

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 120CP: The equilibrium constant for a certain reaction decreases from 8.84 to 3.25 102 when the...

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The equilibrium constant for a certain reaction decreases from 8.84 to 3.25 102 when the temperature increases from 25C to 75C. Estimate the temperature where K = 1.00 for this reaction. Estimate the value of S for this reaction. (Hint: Manipulate the equation in Exercise 79.)
At mom temperature, the equilibrium constant (Kw) for the self-ionization of water is 1.001014. Using this information, calculate the standard free energy change for the aqueous reaction of hydrogen ion with hydroxide ion to produce water. (Hint: The reaction is the reverse of the self-ionization reaction.)
Consider the graph below: (a) Describe the relationship between the spontaneity of the process and temperature. (b) Is the reaction exothermic? (c) S0 (d) At what temperature is the reaction at standard conditions likely to be at equilibrium? (e) Estimate K for the reaction at 97°C.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Acetic acid, CH3CO2H, can form a dimer, (CH3CO2H)2, in the gas phase.. 2CH3CO2H(g)(CH3CO2H)2(g) The dimer is held together by to hydrogen bonds with a total strength of 66.5 kJ per mole of dimer. At 25 C, the equilibrium constant for the dimerization is 1.3103 (pressure in atm). What is ?S for the reaction?
The only stress (change) that also changes the value of K is a change in temperature. For an exothermic reaction, how does the equilibrium position change as temperature increases, and what happens to the value of K? Answer the same questions for an endothermic reaction. If the value of K increases with a decrease in temperature, is the reaction exothermic or endothermic? Explain.
Organ pipes in unheated churches develop tin disease, in which white tin is converted to gray tin. Given white Sm: H f =0.00 kJ/mol; S =51.55 J/mol K gray Sn: H f =2.09 kJ/mol; S =44.14 J/mol K calculate the equilibrium temperature for the transition.
12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant into a lake and estimates that this may warm the water locally to 25 °C. One question to be considered is the effect of this temperature change on the uptake of CO2 by the water. The equilibrium constant for the reaction CO2+H2OH2CO3 ; is K=1.7103 at 25 °C. Because bonds form, the reaction is exothermic. (a) Will this reaction progress further toward products at higher temperatures near the water discharge with its warmer water than it would in the cooler lake water? Explain your reasoning. (b) Carbonic acid has a Kaof 2.5104 at 25 °C. What is the equilibrium constant for the CO2+2H2OHCO3+H3O+? (c) What additional factor should the engineer be considering about CO2 gas, probably before considering this reaction chemistry?
Consider the following relationships: G = 1, H = TS, Q = 1. G = G, K = 1 Which of these relationships is(are) always true for a reaction at equilibrium?
Follow the directions of Problem 27 for each of the reactions in Question 20.
In each of the reactions, how does the equilibrium respond to an increase in pressure? (a) 2SO 2 ( g )+ O 2 ( g ) 2SO 3 ( g ) (b) H 2 ( g )+ I 2 ( g )2HI( g ) (c) 3H 2 ( g )+ N 2 2NH 3 ( g )
. At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide. N2(g)+O2(g)2NO(g)Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations arc found to be [N2]=0.041M. [O2]=0.0078M, and [NO]=4.710M. Calculate the value of K for the reaction.

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