The reversible chemical reactionhas the following equilibrium constant:A+B=C+DKc =[C][D]= 4.1[A][B]Part AInitially, 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)[A] = 0.57Submit Previous Answersfor Part A for Part A do for Part redo foart APart BX Incorrect; Try Again; 2 attempts remaining[D] =SubmitmolLWhat is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M?Express your answer to two significant figures and include the appropriate units.► View Available Hint(s)for Rart B for Part B do for PartValueredo for Part A refor Part A keyboard shortcuts for Part A help for Part AUnitsredo for part B restor Part B keyboard shortcuts for Part B help for Part B Part BBased on a Ke value of 0.250 and the given data table, what are the equilibrium concentrations of XY, X, and Y, respectively?Express the molar concentrations numerically.▸ View Available Hint(s)for Part B for Part B do for Partthredo for Part B reset or Part B keyboard shortcuts for Part B help for Part B[XY], [X], [Y] = 0.372,0.228,0.228Submit Previous AnswersX Incorrect; Try Again; 4 attempts remainingCalculating equilibrium concentrations when the net reaction proceeds in reverseConsider mixture C, which will cause the net reaction to proceed in reverse.Part CThe change in concentration, x, is positive for the reactants because they are produced and negative for the products because they are consumed.Based on a Ke value of 0.250 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?Express the molar concentrations numerically.► View Available Hint(s)for Part Cfor Part Cfor Part Cvec[XY], [X], [Y] = 0.372,0.228,0.228do for PartSubmit Previous AnswersX Incorrect; Try Again; 5 attempts remainingMredo for Part C reset for Part C keyboard shortcuts for Part C help for Part CMConcentration (M) [XY]0.200+x0.200 + xinitial:change:equilibrium:← net1L[X]0.300-x0.300 - x+ [Y]0.300-x0.300 - x

For the following reaction --- A+B⇔C+DEquilibrium constant ,…

The reversible chemical reaction has the following equilibrium constant: A+B=C+D CD K₂=AB= 4.1 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) (A) - 0.57 Submit for Part A for Party do for Part redo foart A relor Part A keyboard shortcuts for Part A help for Part A mol L Part B Previous Answers X Incorrect; Try Again; 2 attempts remaining What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] =2.00 M? Express your answer to two significant figures and include the appropriate units.

The reversible chemical reaction has the following equilibrium constant: A+B=C+D CD K₂=AB= 4.1 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) (A) - 0.57 Submit for Part A for Party do for Part redo foart A relor Part A keyboard shortcuts for Part A help for Part A mol L Part B Previous Answers X Incorrect; Try Again; 2 attempts remaining What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] =2.00 M? Express your answer to two significant figures and include the appropriate units.

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

Consider the reaction: N₂O4 (9) 2NO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: N2(g) + 202 (9) ⇒N₂O4(9) K₁ 1/2N₂(g) + O₂(g) NO₂ (g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K
Part A The reaction below is carried out at a different temperature at which Ke = 0.055. This time, however, the reaction mixture starts with only the product, NO = 0.0100 M, and no reactants. Find the equilibrium concentrations of N2, O2, and NO at equilibrium. N2(8) + O2(g) = 2NO(g) Express your answers to three significant figures separated by commas. > View Available Hint(s) ? [N2]. [O2]. [NO] = М, М, М Submit Provide Feedback Next >
Consider the equilibrium: 2 SO2(g) + O2(g) ⇄ 2 SO3(g) A student places 2.00 moles SO3 in a 1.00 L flask. When equilibrium is reached [O2] = 0.10 M at 130 °C. Calculate the Kc. Hint: use the detectivee method and construct an ICE table. Record your answer as a standard number to 2significant figures. For example, if the answer is 2.75 x 10-3 M then you should enter 0.00275 as the answer.
A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant. A(s)↽−−⇀B(g)+C(g) Then, the container volume was doubled and equilibrium was re‑established. How many moles of A remain? Dont
The chemical equation represents a reversible reaction. 3H2(9) + N2(9) # 2NH3(g) At equilibrium, 1 liter of a mixture of gases at 450°C contains 1.83 mol of hydrogen (H2), 0.793 mol of nitrogen (N2), and 1.72 mol of ammonia (NH3).What is the equilibrium constant for the reaction under these conditions? O A. 0.718 B. 0.609 O C. 1.39 O D. 0.159 96 5 6
2. Given the following equation: A + B = C + D (all gases) If 3.00 moles of A and 3.00 moles ofB are placed in a 2 Liter container and allowed to react to equilibrium with K. = to 9.00, how many moles/L of A, B, C, and D are present at equilibrium. Write the Ke expression and show all work (Hint: do an ICE problem) Aol. O v 1 9:19
Dinitrogen tetroxide partially decomposes according to the following equilibrium: N204(g) = 2NO2(g) A 1.000-L flask is charged with 0.0300 mol of N204. At equilibrium, 0.0204 mol of N204 remains. Calculate the Kc for this reaction. (Enter only the numerical value to three significant figures without units.) Answer:
The reaction A 2 + B 2 =2 AB has an equilibrium constant Kc = 64. The following pictures represent reaction mixtures that contain A 2 molecules (shaded) and B 2 molecules (unshaded), and AB molecules. Which reaction mixture is at equilibrium? 00 (1) (2) (4) reaction mixture (1) reaction mixture (2) reaction mixture (3) reaction mixture (4) O000
A(g) ⇄ 2B(g)Initially, we have 0.914 mol/L of A.What is the concentration of A at equilibrium if the equilibrium constant Kc is equal to 34.7?Give an answer with 4 significant figures.Suggestion: Do not round your answer too much and take the quadratic formula.
7 4 (a) Calculate the value of Kc for the reaction: PC15 (2) PC13 (g) + Cl2 (g) AH = Positive Given that when 8.4 mol of PCls (g) is mixed with 1.8 mol of PC13 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PCls (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (1) Increasing temperature (ii) Lowering the concentration of chlorine (Cl2) (iii) Addition of a catalyst
grade 12 chem: include units, keep work as precise as possible and apply sig figs only to final answers A 2.00 L flask initially contains 2.75 mol of nitrogen gas and 5.50 mol of hydrogen gas. The equilibrium constant for this temperature is 5.75 x 10-5. What are the concentrations of all the compounds when the system has reached equilibrium? N2(g) + 3H2(g) ⇌ 2NH3(g)
The equilibrium constant for the reaction given below can be determined experimentally when known amounts of hydrogen iodide in a sealed tube are heated until equilibrium is attained. 2HI(g) ➡ H2(g) + I2(g) ΔH= -63KJ/mol How is the value of the equilibrium costant affected by: An increase in pressure? Explain. An increase in temperature? Explain.