Homework Answers
Equilibrium constant (Kc) = product of concentration of products to the product of concentration of reactants while each concentration term has a raise to power equal to their stoichiometric coefficient.
As Kc is decreasing with increasing temperature , we can say that concentration of products is decreasing with increasing temperature.
This indicates that reaction equilibrium shifts backward on increasing the temperature and this is the characteristic of an exothermic reaction.
For an exothermic reaction , equilibrium shifts backward on raising the temperature.
dH°rxn for an exothermic reaction is always negative.
So we can conclude that dH°rxn < 0 .
Option (c) is the correct answer.
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5) For a particular chemical reaction it is found that the value for the equilibrium...
5) For a particular chemical reaction it is found that the value for the equilibrium constant...
5) For a particular chemical reaction it is found that the value for the equilibrium constant for the reaction decreases as temperature increases. Based on this we can conclude a) AS rx < 0 b) AS rx c) AH ran d) ΔΗ°κη e) AGºrn > 0 <0
5) For a particular chemical reaction it is found that the value for the equilibrium constant...
5) For a particular chemical reaction it is found that the value for the equilibrium constant for the reaction decreases as temperature increases. Based on this we can conclude a) AH> 0 b) AH 0 c) ASºren > 0 d) AS p < 0 e) AGO
5) For a particular chemical reaction it is found that the value for the equilibrium constant...
5) For a particular chemical reaction it is found that the value for the equilibrium constant for the reaction decreases as temperature increases. Based on this we can conclude a) AH>0 b) AH® < 0 c) AS > 0 d) AS 0 e) AG < 0 6) When 0.0100 moles of dimethyl amine ((CH3)2NH) is added to 1.000 liters of water, the pH of the water increases above the value pH = 7.0 found for neutral solutions. Based on this,...
4) For which of the folling pure chemical substances will SⓇ = 0.0 J/mol K when...
4) For which of the folling pure chemical substances will SⓇ = 0.0 J/mol K when T = 25.0°C? a) O2(g) b) Os(g) c) FeCl(s) d) Both a and e) None of the above 5) For a particular chemical reaction it is found that the value for the equilibrium constant for the reaction decreases as temperature increases. Based on this we can conclude a) AH 0 b) AH > 0 c) AS0 d) AS rx > 0 e) AGºrx <...
4) For which of the folling pure chemical substances will sº = 0.0 J/mol.K when T...
4) For which of the folling pure chemical substances will sº = 0.0 J/mol.K when T = 25.0°C? a) FeCl(s) b) O2(g) c) O3(g) d) Both b and c e) None of the above b) AS 5) For a particular chemical reaction it is found that the value for the equilibrium constant for the reaction decreases as temperature increases. Based on this we can conclude a) AS rxn <0 0 c) AHºrx<0 d) AHºrx>0 <0 e) AGºran
1) What is the value for the van't Hoff factor (i) for Zn(NO:)? a) i =...
1) What is the value for the van't Hoff factor (i) for Zn(NO:)? a) i = 1 b) i - 2 di-4 e)i>4 2) Which of the following makes formation of a solution from two pure chemical substances more likely to occur? a) If randomness increases when a solution forms b) If energy decreases when a solution forms c) If energy increases when a solution forms d) Botha and be e) Both a and 3) For a chemical reaction to...
Unless otherwise specified, you may assume T = 25.0 °C in all of the problems on...
Unless otherwise specified, you may assume T = 25.0 °C in all of the problems on this exam. Part 1. Multiple choice. Circle the letter corresponding to the correct answer. There is one and only one correct answer per problem. [6 points each] 1) Which of the following makes formation of a solution from two pure chemical substances more likely to occur? a) If randomness increases when a solution forms b) If energy decreases when a solution forms c) If...
urgent 4) A particular irreversible chemical reaction follows the rate law rate = k[A] At a...
urgent
4) A particular irreversible chemical reaction follows the rate law rate = k[A] At a particular temperature the value for the rate constant is k - 3.66 x 10-4s. a) In an experiment carried out at that temperature the initial concentration of A in a system is [A]o = 7.66 x 10 M. What will the concentration of A be in the system at t = 400.s? [8 points] b) A plot of Ink vs (1/T) for the rate...
3. If the equilibrium constant for a chemical reaction decreases as the temperature is increases from...
3. If the equilibrium constant for a chemical reaction decreases as the temperature is increases from room temperature to 100 degrees C, would the reaction be exothermic of endothermic? Why?
Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of...
Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N204 is colorless. At High Temperature the red color is strong. || At Low Temperature the gas has less color. If we represent the equilibrium as: 2 NO2(g) = N204(9) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the...
5) For a particular chemical reaction it is found that the value for the equilibrium constant for the reaction decreases as temperature increases. Based on this we can conclude a) AS rx < 0 b) AS rx c) AH ran d) ΔΗ°κη e) AGºrn > 0 <0
5) For a particular chemical reaction it is found that the value for the equilibrium constant for the reaction decreases as temperature increases. Based on this we can conclude a) AH> 0 b) AH 0 c) ASºren > 0 d) AS p < 0 e) AGO
5) For a particular chemical reaction it is found that the value for the equilibrium constant for the reaction decreases as temperature increases. Based on this we can conclude a) AH>0 b) AH® < 0 c) AS > 0 d) AS 0 e) AG < 0 6) When 0.0100 moles of dimethyl amine ((CH3)2NH) is added to 1.000 liters of water, the pH of the water increases above the value pH = 7.0 found for neutral solutions. Based on this,...
4) For which of the folling pure chemical substances will SⓇ = 0.0 J/mol K when T = 25.0°C? a) O2(g) b) Os(g) c) FeCl(s) d) Both a and e) None of the above 5) For a particular chemical reaction it is found that the value for the equilibrium constant for the reaction decreases as temperature increases. Based on this we can conclude a) AH 0 b) AH > 0 c) AS0 d) AS rx > 0 e) AGºrx <...
4) For which of the folling pure chemical substances will sº = 0.0 J/mol.K when T = 25.0°C? a) FeCl(s) b) O2(g) c) O3(g) d) Both b and c e) None of the above b) AS 5) For a particular chemical reaction it is found that the value for the equilibrium constant for the reaction decreases as temperature increases. Based on this we can conclude a) AS rxn <0 0 c) AHºrx<0 d) AHºrx>0 <0 e) AGºran
1) What is the value for the van't Hoff factor (i) for Zn(NO:)? a) i = 1 b) i - 2 di-4 e)i>4 2) Which of the following makes formation of a solution from two pure chemical substances more likely to occur? a) If randomness increases when a solution forms b) If energy decreases when a solution forms c) If energy increases when a solution forms d) Botha and be e) Both a and 3) For a chemical reaction to...
Unless otherwise specified, you may assume T = 25.0 °C in all of the problems on this exam. Part 1. Multiple choice. Circle the letter corresponding to the correct answer. There is one and only one correct answer per problem. [6 points each] 1) Which of the following makes formation of a solution from two pure chemical substances more likely to occur? a) If randomness increases when a solution forms b) If energy decreases when a solution forms c) If...
urgent
4) A particular irreversible chemical reaction follows the rate law rate = k[A] At a particular temperature the value for the rate constant is k - 3.66 x 10-4s. a) In an experiment carried out at that temperature the initial concentration of A in a system is [A]o = 7.66 x 10 M. What will the concentration of A be in the system at t = 400.s? [8 points] b) A plot of Ink vs (1/T) for the rate...
3. If the equilibrium constant for a chemical reaction decreases as the temperature is increases from room temperature to 100 degrees C, would the reaction be exothermic of endothermic? Why?
Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N204 is colorless. At High Temperature the red color is strong. || At Low Temperature the gas has less color. If we represent the equilibrium as: 2 NO2(g) = N204(9) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the...
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