If this is an elementary chemical reaction, then there is a single forward rate and a single reverse rate for this reaction, which can be written as follows:forward rate= |A|B|reverse rate = k₁ [CD]where ky and k, are the forward and reverse rate constants, respectively. When equilibrium is reached, the forward and reverse rates are equal:k[A][B]=k [CD]Thus, the rate constants are related to the equilibrium constant in the following manner:Part Athe forward reaction.For a certain reaction, K, 8.01x102 and k1.64x102 Ms Calculate the value of the reverse rate constant, k. given that the reverse reaction is of the same molecularity asinclude- (multiplication dot) between eachExpress your answer with the appropriate units. Include explicit multiplication within units, for example to enter Mmeasurement.View Available Hint(s)ValueSubmitPart BShow Transcribed Textk₂ = ValueSubmitUnitsPÅY Part CFor a different reaction, K, -95.6, k = 7.42 x 10's, and k, = 77.6s¹ Adding a catalyst increases the forward rate constant to 1.09x10 s What is the new value of thereverse reaction constant, k,, after adding catalyst?Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter Ms include (multiplication dot) between eachmeasurement.View Available Hint(s)2The equilibrium constant wilCE ?UnitsK. ==CDABGincreasedecreaseYet another reaction has an equilibrium constant K 4.32 x 10 at 25°C. It is an exothermic reaction, giving off quite a bit of heat while the reaction proceeds if the temperature israised to 200 C, what will happen to the equilibrium constant?View Avaliable Hint(s)not change

This question belong to Chemical Kinetics. Kc = Kf/Kb,

If this is an elementary chemical reaction, then there is a single forward rate and a single reverse rate for this reaction, which can be written as follows: forward ratek AB reverse rate = k₁ [CD] where ky and ke are the forward and reverse rate constants, respectively. When equilibrium is reached, the forward and reverse rates are equal: k[A][B]=k, [CD] Thus, the rate constants are related to the equilibrium constant in the following manner: Part A For a certain reaction, K, 8.01x102 and k1.64x102 Ms Calculate the value of the reverse rate constant, k,, given that the reverse reaction is of the same molecularity as the forward reaction. k. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M include (multiplication dot) between each measurement. View Available Hint(s) Value Submit → C K₁ = 2- Units CD AB ?

If this is an elementary chemical reaction, then there is a single forward rate and a single reverse rate for this reaction, which can be written as follows: forward ratek AB reverse rate = k₁ [CD] where ky and ke are the forward and reverse rate constants, respectively. When equilibrium is reached, the forward and reverse rates are equal: k[A][B]=k, [CD] Thus, the rate constants are related to the equilibrium constant in the following manner: Part A For a certain reaction, K, 8.01x102 and k1.64x102 Ms Calculate the value of the reverse rate constant, k,, given that the reverse reaction is of the same molecularity as the forward reaction. k. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M include (multiplication dot) between each measurement. View Available Hint(s) Value Submit → C K₁ = 2- Units CD AB ?

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

The following reaction was performed in a sealed vessel at 795 °C: H2 (g) + I2 (g)= 2HI(g) Initially, only H2 and I2 were present at concentrations of H2] = 3.35M and I2 = 2.80M. The equilibrium concentration of I2 is 0.0900 M. What is the equilibrium constant, K , for the reaction at this temperature? Express your answer numerically.
Consider the equilibrium system described by the chemical reaction below. Determine the concentration of O2 at equilibrium by writing the equilibrium constant expression and solving it. Complete Parts 1-2 before submitting your answer. 2 H2O(g) 2 H2(g) + O2(g) 1 2 NEXT At this temperature, the Kc = 2.4 × 10-3 and the equilibrium concentrations of H2O and H2 are 0.11 M and 0.019 M, respectively. If [×] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Ко = = 2.4 × 10-3 RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11]² [0.019]² [x] [x]² [2x] [2x]2
For the reaction 4PH3(g)↽−−⇀6H2(g)+P4(g)4PH3(g)↽−−⇀6H2(g)+P4(g) the equilibrium concentrations were found to be [PH3]=0.250 M,[PH3]=0.250 M, [H2]=0.400 M,[H2]=0.400 M, and [P4]=0.750 M.[P4]=0.750 M. What is the equilibrium constant for this reaction?
For which of the following reactions is it NOT important that the species collide with the correct orientation? 2 NO(g) + O2(g)* -->2 NO2(g) OHCl(g) + H₂O (1) ---> H30* (aq) + Cl(aq) Ag* (aq) + Cl(aq) --> AgCl(s) 2 H2(g) + O2(g) -> 2 H₂O (1)
2 AB2 (aq) + C2 (aq) <-> 2 AB2C(aq) is an endothermic reaction that has reach equilibrium. If the system is heated, will the concentration of C2 increase, decrease, or not change?
6) Given the reaction: A(aq) + B(aq) = 2C(aq) + D(aq). 2.00 moles of each reactant were dissolved into 1.00 liter of water. The reaction reached equilibrium, and at equilibrium the concentration of A was 1.60 M. A) Calculate the equilibrium concentrations for each substance. B) Write the equilibrium constant expression. [c]²[0] Kc = [A] [B] C) Calculate the value for the equilibrium constant, Keq.
Nickel carbonyl decomposes to form nickel and carbon monoxide, like this: Ni (CO),(9)- Ni(s)+4 CO(g) At a certain temperature, a chemist finds that a 9.1 L reaction vessel containing a mixture of nickel carbonyl, nickel, and carbon monoxide at equilibrium has the following composition: compound amount Ni(CO)4| 0.555 g Ni 48.3 g CO 1.92 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K _ = | x10
The progress with time of a reaction system is depicted in the figure here. Red spheres represent the molar concentration of substance A, and blue spheres represent the molar concentration of substance B. What is the value of the equilibrium constant Kc?
The equilibrium constant for the reaction 2 KAl(OH)4(aq) + 4 H2SO4(aq) ⇆ 2 KAl(SO4)2(s) + 8 H2O(l) at room temperature is 84.5. At equilibrium, the concentration of sulfuric acid (H2SO4) is 0.531M. What is the concentration of KAl(OH)4 (in moles/L)?
When chlorine gas is reacted with bromine gas an equilibrium will be established with bromine monochloride: Br2(g) + Cl2(g) 2BrCl(g)
Select the single best answer. For the synthesis of ammonia N2(g) + 3H,(g) 2NH3(g) the equilibrium constant K. at 375°C is 1.2. Starting with [H,lo = 0.76 M, [N2lo = 0.60 M and [NH3]0 = 0.48 M, which concentration(s), if any, will have increased when the mixture comes to equilibrium? H2 N2 N2 and H, NH3 There will be no change