Activity 3: Fill in the blanks with the correct answer. Imagine that you have a system that is already at equilibrium. a. If you add more reactant to the mixture, the equilibrium will shift to the b. If you add more products to the mixture ,the equilibrium will shift to the c. If you remove the reactants from the mixture, the equilibrium will shift to the If you will remove the product from the mixture, the equilibrium will shift to the d. e. When there is a shift in the equilibrium position at constant temperature, will the value of K be changed? f. Changing the is the only way to change the value of K.

Activity 3: Fill in the blanks with the correct answer. Imagine that you have a system that is already at equilibrium. a. If you add more reactant to the mixture, the equilibrium will shift to the b. If you add more products to the mixture ,the equilibrium will shift to the c. If you remove the reactants from the mixture, the equilibrium will shift to the If you will remove the product from the mixture, the equilibrium will shift to the d. e. When there is a shift in the equilibrium position at constant temperature, will the value of K be changed? f. Changing the is the only way to change the value of K.

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Given the Equilibrium Equation: CO (g) + Cl2 (g) <--> COCl2 (g) and ΔH = -25.9 kcal/mole Which option would make the equilibrium shift towards the products? Pick all that apply. (There may be multiple answers that are correct) a. adding more phosgene b. adding more carbon monoxide c. increasing the temperature d. decreasing the reaction container volume e. decreasing the temperature
Consider this equilibrium N₂(g) + H₂(g) NH3(g) + 94 kJ The equilibrium law expression for the balanced chemical equation would be A. [N₂][H₂]/[NH3] [NH3]2/[H₂]³[N₂] B. [NH3] [H₂][N₂] 2[NH3]2/3 [H₂]³[N₂] C. [NH3]2/[H₂][N₂] D. E.
Which of the following is incorrect? A. When pressure, volume, or concentration is changed, the equilibrium position may be altered. B. When pressure, volume, or concentration is changed, the value of the equilibrium constant does not change. C. A change in temperature does not alter the equilibrium constant. D. Adding a catalyst to a reaction only causes the mixture to reach equilibrium faster.
If we represent the equilibrium as: 2 NO2(g) = N204(g) 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 temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of NO2: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
A mixture of CO and Cl2 is placed in a reaction flask: [CO] = 0.0103 M and [Cl2] = 0.00610 M. At equilibrium, the concentration of Cl2 is 0.00311 M. Using an ICE table, calculate the equilibrium concentration of CO. a. 0.00731 M b. 0.00311 M c. 0.0103 M d. 0.0206 M e. 0.00299 M
Equilibrium is reached in a chemical reaction when A. the reactants are completely consumed. B. the concentrations of all reactants and products become equal. C. the rates of the opposing reactions become equal. D. the forward and reverse reactions stop.
Given each equilibrium constant, state whether the reactants are favored, the products are favored, or both the reactants and products are present at equilibrium. a. 5.0 × 10 −4 b. 4.4 × 10 5 c. 350 d. 0.35
Hey, im a little stuck on this sheet :)
d. Suppose you add compound E to the equilibrium mixture. Compound E reacts with compound D which is a component of the equilibrium to form compound F as described in the equation below. E + D Which compound is removed from the equilibrium mixture when you add compound E to the mixture? (Enter "correct" for ALL correct answers.) • B D e. What shift in the equilibrium will occur as a result of the addition of compound E? (Enter "correct" for the correct shift.) A + B C + D (shift to the right) A + B C + D (shift to the left)
I. 2NOCl (g)< < > 2NO(g) + Cl2(g) K= 1.6X 10-5 II. 2NO (g) < > N2(g) + O2(g) K= 1.0 X 1031 Which of the following will you choose to generate the most amount of NO? (Think which of the reactions will favor the formation of NO.)a.Forward reaction of IIb.Forward reaction of Ic.Reverse reaction of Id.Reverse reaction of II
Chamber A contains 40% oxygen and Chamber B contains 20% oxygen. Chambers are connected by a tube and the oxygen molecules are free to cross. Which of the following is most likely to occur over time? A. all of the oxygen will move into chamber B B. The oxygen concentration will remain the same of both sides C. Some oxygen will move chamber A to chamber B until equilibrium reached D. Some oxygen will move chamber B to chamber A until one side has more oxygen
f the value of Q is greater than K for an equilibrium reaction then a. a catalyst is necessary to achieve equilibrium. b. the reaction will proceed to the right until equilibrium is established. c. the reaction will proceed to the left until equilibrium is extablished. d. the reaction will go left or right depending on the reaction stoichiometry. e. Both (a) and (d) are correct.