We know whether or not if the forward or the backward reaction are favored due to...
We know whether or not if the forward or the backward reaction are favored due to comparing Qc and Kc. Now when do you know the reaction is at equilibrium by just looking at the concentrations? Is this possible? If not, how is the Kc found for each problem? I know how to calculate the Kc with equilibrium concentrations, but you need one or the other. It always says it favors a direction and will keep favoring that reaction until the system is at equilibrium, but when does it stop favoring one side and the system hits equilibrium? I'm sorry in advanced! I am very lost!!!!
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We know whether or not if the forward or the backward reaction
are favored due to...
1. Which of the following is true for a chemical reaction at equilibrium? only the forward...
1. Which of the following is true for a chemical reaction at equilibrium? only the forward reaction stops only the reverse reaction stops both the forward and reverse reactions stop the rate constants for the forward and reverse reactions are equal the rates of the forward and reverse reactions are equal 2. A chemical equilibrium may be established by starting a reaction with reactants only. d. any quantities of reactants and products. products only. e. all the above equal quantities...
I just did a lab on determination of an equilibrium constant through the reaction EtAc (aq)...
I just did a lab on determination of an equilibrium constant through the reaction EtAc (aq) + H2O (sln) <-> EtOH (aq) +HAc (aq). For all initial concentrations, K was less than one. Which I know says that equilibrium favors reactants. One of the post lab questions is "Is the hypothesis that the equilibrium constant, K, really a constant not dependent on the initial concentrations correct? Explain your answer. " I am not sure how to answer this
I just did a lab on determination of an equilibrium constant through the reaction EtAc (aq)...
I just did a lab on determination of an equilibrium constant through the reaction EtAc (aq) + H2O (sln) <-> EtOH (aq) +HAc (aq). For all initial concentrations, K was less than one. Which I know says that equilibrium favors reactants. One of the post lab questions is "After the titration of the solutions at equilibrium, how will the solution return to equilibrium? Which chemicals will increase and which will decrease? (Be careful with acetic acid) " I am not...
I just did a lab on determination of an equilibrium constant through the reaction EtAc (aq) + H2O...
I just did a lab on determination of an equilibrium constant through the reaction EtAc (aq) + H2O (sln) <-> EtOH (aq) +HAc (aq). For all initial concentrations, K was less than one. Which I know says that equilibrium favors reactants. One of the post lab questions is "After the titration of the solutions at equilibrium, how will the solution return to equilibrium? Which chemicals will increase and which will decrease? (Be careful with acetic acid) " I am not...
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant Kc. 3A...
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant Kc. 3A + 2B -><- 4C kc=3.13x10^29 If at this temperature, 2.50 mol of A and 3.70 mol of B are placed in a 1.00L container, what are the concentrations of A, B, C at equilibrium? I know the answer to B and C but system is keep telling me A is wrong The answer I have is [A]=0 <--- wrong [B]=2.033 <--- correct [C}=3.333 <----...
Using stock bottles of CaCl2 and KOH solutions, a student prepared a 1.00L solution mixture which...
Using stock bottles of CaCl2 and KOH solutions, a student prepared a 1.00L solution mixture which contained, before any reaction occurred, [Ca2+] = 0.075M and [OH–] = 0.085M. After mixing the solution, a precipitate of Ca(OH)2 (s) was formed (reaction occurred in the right-to-left direction). The student then added a further 1.00L of water and stirred; the precipitate disappeared— all the solid had redissolved. Which one of the following is a possible value for the equilibrium constant, Kc, of this...
UULUUI VULL I TULU Cui suujell wiele we just memorize a collection of facts. That is...
UULUUI VULL I TULU Cui suujell wiele we just memorize a collection of facts. That is almost useless. To learn science, to succeed in scientific fields is to see how all of the ideas relate to each other. The more connections you can establish, the more you can use what you know and the easier it is to remember. Indulge me for just a single question. Select all of the following that are true about disturbing an equilibrium (Le Chatelier's...
The general form of a chemical reaction is aA + bB = cC +dD Where A...
The general form of a chemical reaction is aA + bB = cC +dD Where A and B are reactants in the forward direction and C and D are products in the forward direction. The lower case letters are the stoichiometric coefficients for the balanced equation. The general form of the equilibrium constant equation is then: Keq = [C]c[D]d/[A]a[B]b Part I: Q vs. K Q: reaction quotient can be calculated for a reaction at any concentration values of reactants and...
please i need quick help these questions are due so soon and i dont know the answers please help me thanks . Que...
please i need quick help these questions are due so soon and i
dont know the answers please help me thanks .
Question Completion Status: QUESTION Consider the following acid-base reaction. Equilibrium for this reaction lies to the: OH H-CEC + H-CEC-H + A. right. B. Equilibrium favors neither forward nor reverse reaction. O C. left. D. It cannot be determined. QUESTION 2 Does the equilibrium of this reaction lie to the left or right? BF OH BF3 + A,...
Consider the following reaction for Questions 1.3 and answer the questions based upon this GU u...
Consider the following reaction for Questions 1.3 and answer the questions based upon this GU u IIULS reaction: CÓ (g) + 3 H (g) + CH4 (g) + H2O (G) 1. At 25°C, Keq=4.0. What must be the Co] at equilibrium If the equilibrium concentrations of [H.]= 2.0M. (CH) = 5.0M, and (HO) = 3.OM? Answer: 0.469 M The ICE table is a way to keep track of what is happening in the reaction vessel. The initial concentrations if given...
1. Which of the following is true for a chemical reaction at equilibrium? only the forward reaction stops only the reverse reaction stops both the forward and reverse reactions stop the rate constants for the forward and reverse reactions are equal the rates of the forward and reverse reactions are equal 2. A chemical equilibrium may be established by starting a reaction with reactants only. d. any quantities of reactants and products. products only. e. all the above equal quantities...
UULUUI VULL I TULU Cui suujell wiele we just memorize a collection of facts. That is almost useless. To learn science, to succeed in scientific fields is to see how all of the ideas relate to each other. The more connections you can establish, the more you can use what you know and the easier it is to remember. Indulge me for just a single question. Select all of the following that are true about disturbing an equilibrium (Le Chatelier's...
please i need quick help these questions are due so soon and i
dont know the answers please help me thanks .
Question Completion Status: QUESTION Consider the following acid-base reaction. Equilibrium for this reaction lies to the: OH H-CEC + H-CEC-H + A. right. B. Equilibrium favors neither forward nor reverse reaction. O C. left. D. It cannot be determined. QUESTION 2 Does the equilibrium of this reaction lie to the left or right? BF OH BF3 + A,...
Consider the following reaction for Questions 1.3 and answer the questions based upon this GU u IIULS reaction: CÓ (g) + 3 H (g) + CH4 (g) + H2O (G) 1. At 25°C, Keq=4.0. What must be the Co] at equilibrium If the equilibrium concentrations of [H.]= 2.0M. (CH) = 5.0M, and (HO) = 3.OM? Answer: 0.469 M The ICE table is a way to keep track of what is happening in the reaction vessel. The initial concentrations if given...
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