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Given the following pKa values, what can be determined about the given reaction? (pKa of H3PO4...
For each of the following reactions, use the pKa values given in the Table to predict...
For
each of the following reactions, use the pKa values given in the
Table to predict whether reactants or products are favored at
equilibrium.
For each of the following reactions, use the pKa values given in the Table to predict whether reactants or products are favored at equilibrium Compound Hydronium ion (H30*) Dichloroacetic acid (C2H202Cl2) Dihydrogen sulfide (H2S) Phenol (C6H5OH) Piperidinium ion (C5H12N*) Water (H20) pKa 1.7 1.35 7.0 10.0 11.2 15.7 Drag the appropriate items to their respective bins....
48. If the conversion of A to B is slow and B to C is fast, what is the rate equation for this reaction? A) Rate =...
48. If the conversion of A to B is slow and B to C is fast, what is the rate equation for this reaction? A) Rate = K[(CH3CHCI][H20] B) Rate - K[(CH3)2CHCI] C) Rate = K[(CH3)CH] [H0] D) Rate = {[(CH3)2CH] 49. Which of the following statements about a catalyst is true? A) A catalyst accelerates a reaction by changing the amount of reactant and product at equilibrium B) A catalyst accelerates a reaction by lowering the energy of activation...
For a particular reaction K = 98000. What can be said about this reaction? A) There...
For a particular reaction K = 98000. What can be said about this reaction? A) There are many more products than reactants in the equilibrium mixture. B) There are many more reactants than products in the equilibrium mixture. C) There are roughly equal amounts of reactants and products in the equilibrium mixture. D) The reaction has not yet reached equilibrium because K does not equal 1.
D Question 2 1 pts Which statement(s) concerning the reaction is/are true? 2A) A2(g) +B2(g) K-29x...
D Question 2 1 pts Which statement(s) concerning the reaction is/are true? 2A) A2(g) +B2(g) K-29x 10-85 There are fewer moles of reactants than products at equilibrium, because the equilibrium constant is small. There are more moles of reactants than products at equilibrium, because the equilibrium constant is large. There are near equal amounts of reactants and products at equilibrium because the equilibrium constant is close to 1 There are more moles of reactants than products at equilibrium, because the...
Documenti Student ID 4. Which of the following is true about the reaction quotient? . None...
Documenti Student ID 4. Which of the following is true about the reaction quotient? . None of these answers are correct It relates the concentrations of products to reactants at any point in time. It can never be equal to the equilibrium constant. It is always equal to the equilibrium constant. It relates the ratio of the concentrations of products to reactants once the reaction has reached chemical equilibrium. . • 5. Which of the following is true about the...
Question 2 1 pts Which statement(s) concerning the reaction is/are true? 2ABig) Alg) + Bale) K-2.9...
Question 2 1 pts Which statement(s) concerning the reaction is/are true? 2ABig) Alg) + Bale) K-2.9 x 10-85 There are fewer moles of reactants than products at equilibrium, because the equilibrium constant is small There are more moles of reactants than products at equilibrium, because the equilibrium constant is large. There are near equal amounts of reactants and products at equilibrium because the equilibrium constant is close to 1 There are more moles of reactants than products at equilibrium, because...
Equilibrium and Le Chatelier Principle In an endothermic reaction what is correct about the energy in...
Equilibrium and Le Chatelier Principle
In an endothermic reaction what is correct about the energy in the reaction? O Energy becomes available Energy is absorbed O The energy stays the same O The reaction needs to be kept cold O Only one component realeases energy What is the main difference between a reversible and irreversible reaction? O Both a irreversable and a reversible make products are formed but not reactants irreversable reaction the products cannot convert back to the reactants,...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) +...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g)...
6. Which of the following statements is not true? A) Bond breaking is endothermic. B) The...
6. Which of the following statements is not true? A) Bond breaking is endothermic. B) The bond dissociation energy for bond breaking is always negative. C) Bond making is exothermic. D) The bond dissociation energy for bond formation is always negative. 37. Using the bond dissociation energies given, calculate AH® for the following reaction. CH,CH -Br + H2O CH,CH-OH + HBr AH KJ/mol Bond A-B CH3CH2-Br H-OH сHCH-он H-Br A) +108 KJ/mol B) -130 KJ/mol C) -22 KJ/mol D) +22...
For the reaction H2(g)+I2(g)⇌2HI(g), K= 57.0 at 700 K what can be said about this reaction...
For the reaction H2(g)+I2(g)⇌2HI(g), K= 57.0 at 700 K what can be said about this reaction at this temperature? For the reaction , at 700 what can be said about this reaction at this temperature? The equilibrium lies far to the right. The reaction will proceed very slowly. The reaction contains significant amounts of products and reactants at equilibrium. The equilibrium lies far to the left.
For
each of the following reactions, use the pKa values given in the
Table to predict whether reactants or products are favored at
equilibrium.
For each of the following reactions, use the pKa values given in the Table to predict whether reactants or products are favored at equilibrium Compound Hydronium ion (H30*) Dichloroacetic acid (C2H202Cl2) Dihydrogen sulfide (H2S) Phenol (C6H5OH) Piperidinium ion (C5H12N*) Water (H20) pKa 1.7 1.35 7.0 10.0 11.2 15.7 Drag the appropriate items to their respective bins....
48. If the conversion of A to B is slow and B to C is fast, what is the rate equation for this reaction? A) Rate = K[(CH3CHCI][H20] B) Rate - K[(CH3)2CHCI] C) Rate = K[(CH3)CH] [H0] D) Rate = {[(CH3)2CH] 49. Which of the following statements about a catalyst is true? A) A catalyst accelerates a reaction by changing the amount of reactant and product at equilibrium B) A catalyst accelerates a reaction by lowering the energy of activation...
For a particular reaction K = 98000. What can be said about this reaction? A) There are many more products than reactants in the equilibrium mixture. B) There are many more reactants than products in the equilibrium mixture. C) There are roughly equal amounts of reactants and products in the equilibrium mixture. D) The reaction has not yet reached equilibrium because K does not equal 1.
D Question 2 1 pts Which statement(s) concerning the reaction is/are true? 2A) A2(g) +B2(g) K-29x 10-85 There are fewer moles of reactants than products at equilibrium, because the equilibrium constant is small. There are more moles of reactants than products at equilibrium, because the equilibrium constant is large. There are near equal amounts of reactants and products at equilibrium because the equilibrium constant is close to 1 There are more moles of reactants than products at equilibrium, because the...
Documenti Student ID 4. Which of the following is true about the reaction quotient? . None of these answers are correct It relates the concentrations of products to reactants at any point in time. It can never be equal to the equilibrium constant. It is always equal to the equilibrium constant. It relates the ratio of the concentrations of products to reactants once the reaction has reached chemical equilibrium. . • 5. Which of the following is true about the...
Question 2 1 pts Which statement(s) concerning the reaction is/are true? 2ABig) Alg) + Bale) K-2.9 x 10-85 There are fewer moles of reactants than products at equilibrium, because the equilibrium constant is small There are more moles of reactants than products at equilibrium, because the equilibrium constant is large. There are near equal amounts of reactants and products at equilibrium because the equilibrium constant is close to 1 There are more moles of reactants than products at equilibrium, because...
Equilibrium and Le Chatelier Principle
In an endothermic reaction what is correct about the energy in the reaction? O Energy becomes available Energy is absorbed O The energy stays the same O The reaction needs to be kept cold O Only one component realeases energy What is the main difference between a reversible and irreversible reaction? O Both a irreversable and a reversible make products are formed but not reactants irreversable reaction the products cannot convert back to the reactants,...
6. Which of the following statements is not true? A) Bond breaking is endothermic. B) The bond dissociation energy for bond breaking is always negative. C) Bond making is exothermic. D) The bond dissociation energy for bond formation is always negative. 37. Using the bond dissociation energies given, calculate AH® for the following reaction. CH,CH -Br + H2O CH,CH-OH + HBr AH KJ/mol Bond A-B CH3CH2-Br H-OH сHCH-он H-Br A) +108 KJ/mol B) -130 KJ/mol C) -22 KJ/mol D) +22...
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