5. Consider the following reaction:2A+BCA kinetics study on this reaction yielded the following data:[A] mol/L[B] mol/LRate = mol/L/s0.02500.04004.06 x 10-30.02500.08004.06 x 10-30.05000.08004.06 x 10-3Calculate the K constant for the above reaction: ()+(p) 28 aa. 0.025 mol/L.sevodsAb. 0.0010 mol/L.sc. 0.0020 mol/L.sd. 0.00406 mol/L. se. None of the above(p) 2 + (p) OS (2):82svods evil to onaitevodsall brisang wond6. Calculate AG° for the following reaction:Thiog2 SO2(g) + O2(g) → 2 SO3(g)AGf in kJ/moles for SO2(g) is -300.2, for SO3(g) is -371.1 and for O2 is 0.0.a. +141.8 kJb. +70.9 kJc. #70.9 kJenimmetedd. -141.8 kJlomEL7. Consider the following reaction for the production of SO3:18.8XC70 b2 SO2(g) + O2(g) → 2 SO3(g)Which of the following expressions best illustrates the rate of the product?a. rate = 2A[SO3] / Atb. rate = A[SO3]/2Atc. rate = 2A[SO3]/2AtプラFRASER

Answered: 5. Consider the following reaction:…

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...

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1- The reaction between sulfur dioxide and molecular oxygen has a Kc value of 1.7 x 106 at 700 K. 2SO2 (g) + O2 = 2SO3 If this reaction is carried out in a sealed reaction vessel and the equilibrium concentrations of O, and SO3 are 2.1 x 10-3 M and 3.8 M, respectively, then what is the concentration of SO2 in the vessel at equilibrium? 2- Consider the following equilibrium 2SO3 (g) + 2SO2 (g) = 02 (g) Suppose that 0.0150 mol SO3 (g) is placed in a 1.00 L vessel and allowed to come to equilibrium at a high temperature. When equilibrium is achieved, 0.0076 mol SO3 remains. Calculate the value of the equilibrium constant for the reaction. (Hint: use ICE table)
7.
MISSED THIS? Read Section 16.8 (Pages 701 - 710); Watch KCV 16.8, IWE 16.9. Consider the following reaction and associated equilibrium constant: aA (g) + bB (g) = cC (g) Kc = 3.0 Part A Find the equilibrium concentrations of A, B, and C for a = 1, b = 1, and c = 2. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction. Express your answer using two significant figures. Enter your answers separated by commas. [A], [B]. [C] = Submit Part B X Incorrect; Try Again; 3 attempts remaining IV—| ΑΣΦ 5 Previous Answers Request Answer [A], [B], [C] = Submit Find the equilibrium concentrations of A, B, and C for a = 1, b = 1, and c = 1. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction. Express your answer using two significant figures. Enter your answers separated by commas. OF IVE ΑΣΦ Request Answer ? www M ? M
The equilibrium constant for the reaction shown below is K = 1.3 x 10-37. Fe(CN)64-(aq) ⇌⇌ Fe2+(aq) + 6 CN-(aq) If a solution is prepared with initial concetration of [Fe(CN)64-] = 1.00 mol L-1, what will be the equilibrium concentration of Fe2+?
The following reaction is at equilibrium and being monitored by a chemist: . 2NOF (g) 2NO(g) + F2 (g). The chemist measures these concentrations at equilibrium: ● [NOF] = 0.56 M [NO] 0.32 M . [F₂] = 0.28 M What is the equilibrium constant for this reaction? 0.16 M O 0.051 M² 1.2 M 15 M 0.091 M O
7
A sample of HI was placed in a container and the following reaction was allowed to come to equilibrium. =2 H2(g) +12(g) 2 HI(g) The equilibrium concentrations were found to be [HI] = 3.88 M and [H2] = [12] = 0.556. Calculate the equilibrium constant, Kc, for the reaction. Note Kc is often called K. esc of F1 - F2 80 F3 F4 2 @ #3 3 Q W L $ S4 F5 % 0105 MacBook Air 66 F6 & 7 F7
The reaction N2(g) + O2(g) -> 2 NO(g) comes to equilibrium. The concentrations of each component are measured. They are: [N2] = 1.5 x 10-3 [02] = 2.3 x 102 [NO]= 4.0 x 10-3 The value of Kc is. Oa. 0.46 Ob. 1,2x 102 Oc. C. 2.1 8.7 x 10-3
it's not 1.33 either
Consider the following heterogenous reaction: 2AB(s) + C3(aq) + 4D(aq) ⇌ 2ABCD(aq) + CD2(l) The initial concentration of C3 is 0.20 M and 0.10 M for D. 5.0 g of reactant AB was also added. There were no products in the reaction flask at time 0. At equilibrium, the [D]eq = 0.03 M. (i) Will the concentration of reactant AB and product CD2 affect equilibrium? Explain why or why not. (i) Calculate the equilibrium constant, Kc for this reaction.
In air at 25 °C and 1.00 atm, the N₂ concentration is 0.01 M and the O₂ concentration is 0.033 M. The reaction N₂(g) + O₂(g) → 2NO(g) has Kc = 4.8 x 10-³1 at 25 °C. Taking the N₂ and O₂ concentrations given above as initial values, calculate the equilibrium NO concentration that should exist in our atmosphere from this reaction at 38 °C, Kc = 1.0E-29. Make simplifying assumptions in your calculations. (Express your answer in scientific notation.) [NO] = i M
1

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