Review I Consta The reversible chemical reaction A+B=C+D Part A as the following equilibrium constant: |C]D] K. = [AB] = 4.5 Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Express your answer to two significant figures and include the appropriate units. > View Available Hint(s) HẢ ? [A] = Value Units Submit Part B What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 Mand B =2.00 M ? Express your answer to two significant figures and include the appropriate units > View Available Hint(s) HẢ ? [D] = Value Units Submit

Review I Consta The reversible chemical reaction A+B=C+D Part A as the following equilibrium constant: |C]D] K. = [AB] = 4.5 Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Express your answer to two significant figures and include the appropriate units. > View Available Hint(s) HẢ ? [A] = Value Units Submit Part B What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 Mand B =2.00 M ? Express your answer to two significant figures and include the appropriate units > View Available Hint(s) HẢ ? [D] = Value Units Submit

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

ACTIVITY 1: Let's Practice: In this activity answer some following problems and proof if the reaction is going forward or reverse. (On a Piece of Paper) Write the equilibrium constant expression, Kc, for the following reactions. А. Indicate also if the equilibrium is homogeneous or heterogeneous. A. 2 Ag(9) + Zntaa) = 2 Agčaa) + Zns) B. 2 C,H4c9) + 2 H20zc@) = C2H6(9) + 0zc@) C. Cs) + 2 HA@)= CH«@) D. 4 HCl(aq) + 0z(9) = 2 H201) + 2 Clz®)
Submit Part B Consider the reaction, which takes place at a certain elevated temperature CO(g) + NH3(g)= HCONH2 (g), K. = 0.880 If a reaction vessel initially contains only C0 and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of HCONH2 be at equilibrium? Express your answer with the appropriate units. • View Available Hint(s) HÀ [HCONH2] = Value Units Submit Next> Provide Feedback MacBook Air
Predict the equilibrium concentration of Ca²+ in the reaction described below by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. NEXT > A solid sample of CaCrO dissolves in solution. Fill in the ICE table with the appropriate value for each involved species to determine the pressure of all reactants and products. 4 Initial (M) Change (M) Equilibrium (M) 7.1 x 104 - x 0 7.1 x 104 + 2x CaCrO₂(s) Ca²+(aq) + CrO²(aq) 1 CaCrO (s) 7.1 x 10-4 7.1 x 104 - 2x +X 2 11 -X Ca²+ (aq) +2x 3 + -2x CrO² (aq) RESET 7.1 × 10-¹4 + x
Examine the following equilibrium table for the reaction shown at the top of the table. COog) + H,O(g) CO-(g) H;(g) Initial concentrations (M) 0.0600 0.0600 0.100 0.100 Changes in concentrations (M) Equilibrium concentrations (M) If at the temperature of the reaction container, Q < K¢ what value should be placed in the table for the equilibrium concentration of O 0.100 -x O 0.0600 +x O -x O +x O 0.100 +x O 0.0600 - x
in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working!!!!!!!
Consider the following reaction at a certain temperature: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) An equilibrium mixture contains 1.2 mol Fe, 0.0010 mol O2, and 2.0 mol Fe203 all in a 2.0-L container. Calculate the value of K for this reaction. K = Submit Answer Try Another Version 10 item attempts remaining
Answer letter d and e
Answer 1, 2 and 3
Activity 1. Write the Expression. (LAS 5.b) Learning Objectives: Write equilibrium constant expression for a given balanced chemical equation for homogeneous and heterogeneous equilibria. What you need: pen and paper Whattodo: Identify if the equilibrium is homogeneous or heterogeneous. Write both K, and Kp for each reversible reaction. Homogeneous/ Heterogeneous Reversible Reaction Ke Kp 1) 2SO2 (g) + O2 (g) = 2 SO3 (g) 2) 2NH3 (g) + H2SO, (1) – (NH,)-SO4 (s) 3) S (s) + H,SO, (aq) = H,S¿O, (aq) 4) CH4 (g) + 2H2S (g) = CS2 (g) + 4H2 (g) 5) C (s) + 2H2 (g) = CH4 (g)
Question 10 In an experiment where the initial concentration of Fe3+ was 0.00133 M and the initial concentration of SCN* was 0.000468 M, a student measured the final equilibrium concentration of FENCS2* to be 0.000177 M. Fe3*(aq) + SCN'(aq) FENCS2*(aq) Calculate the final equilibrium concentration of SCN'. Your Answer: Answer
Question 5 Please help
Solve 10 in a chart please like the picture