5. Consider the reaction below. If the reaction is uncatalyzed k=10's', if it is catalyzed k₁ = 10's'. For the uncatalyzed reaction k=10³s¹. k₁ k₁ a) What is K for the uncatalyzed reaction? cq b) Does it change for the catalyzed reaction? Why or why not? 5. If the middle line (darker one) is the rate of an enzyme reaction in the presence of an uncompetitive inhibitor, which line number represents the reaction without the inhibitor? Explain your answer. [S] 7. Draw a Lineweaver-Burk plot of the graph in the previous question. Values are not necessary just comparative shapes of lines. (Label axis and y intercept)

5. Consider the reaction below. If the reaction is uncatalyzed k=10's', if it is catalyzed k₁ = 10's'. For the uncatalyzed reaction k=10³s¹. k₁ k₁ a) What is K for the uncatalyzed reaction? cq b) Does it change for the catalyzed reaction? Why or why not? 5. If the middle line (darker one) is the rate of an enzyme reaction in the presence of an uncompetitive inhibitor, which line number represents the reaction without the inhibitor? Explain your answer. [S] 7. Draw a Lineweaver-Burk plot of the graph in the previous question. Values are not necessary just comparative shapes of lines. (Label axis and y intercept)

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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10. The rate law of the overall reaction is k[A][B]0. Which of the following will not increase the rate of the reaction? A. increasing the concentration of reactant AB. increasing the concentration of reactant B C. increasing the temperature of the reaction D. adding a catalyst for the reaction 11. Which of the following would NOT increase the rate of reaction? A. raising the temperature B. adding catalyst C. increasing the volume of the container D. increasing the concentration of the reactants 12. What is the correct expression of the rate of a chemical reaction? A. grams per mole B. energy consumed per mole C. molarity per second D. volume of gas per unit time 13. Why an increase in temperature increases a reaction rate? A. only because there are more collisions B. only because the particles collide with greater energy C. by providing an alternative pathway for the reaction to follow D. because the particles collide more frequently and with greater energy 14. Which condition…
How do you solve HWK1?
Label each reactant and product in the given chemical reaction. R F V CH4 96 5 G Search or type URL T + 20₂ G B tv 6 Y H Answer Bank product MacBook Pro N 9 U J CO₂ reactant 00 M 1 K ģ 69 + I O 2H₂0 L O command P Λ' : ; I option { [ ? = 1 O I } 1 dele
we now have: Step 1: Fast, reversible HA = H+ + A- Step 2: Fast, reversible X + H+ = HX+ Step 3: Slow HX+ = productsrate= k3 k2/k-2 [X][HX+] Does the current rate law contain an intermediate?
3. Dinitrogen tetroxide, N2O4, dissociates at room temperature to give nitrogen dioxide, NO2. N2O4 (g) = 2 NO2 (g) The equilibrium constant Kç at 25°C is 0,125. What percentage of dinitrogen tetroxide is dissociated when 0,0300 mol N204 is placed in a 1,00 dm3 flask and left to reach equilibrium? (а) (b) The amount of nitrogen dioxide formed increases as the temperature rises. Is the dissociation of N2O4 endothermic or exothermic?
Indicate whether the equilibrium will shift RIGHT (products), LEFT (reactants), or NOT AT ALL for the following reactions when the given stress is applied. Zn(s) + 2HCI(I) ⇒ ZnCl₂(s) + H₂(g) + Heat (EXO) Adding Zn Adding HCI Adding ZnCl2 Adding H2 Removing H2 Removing Zn Increasing Temp Decreasing Temp Increasing Pressure Decreasing Pressure
Please show all your work please, thank you! Sorry, this question has many parts. The reaction O3(g)+O(g)→2O2(g), occurs via the following mechanism:Step 1: Cl(g)+ O3(g)→ClO(g)+O2(g); Ea=85 kJ/molStep 2: ClO(g)+ O(g)⇌Cl(g)+O2(g); Ea=10 kJ/mol Using the proposed mechanism, derive a rate law. *Hint: use the activation energies to determine the slower step. Show all of your work.
5. The reaction between calcium carbonate and hydrochloric acid is shown. CaCO3(s) + 2 HCI(aq) CaCl2{ag) + H2O(m + CO2(9) Which would increase the reaction rate between calcium carbonate and hydrochloric acid? O crushing the calcium carbonate into a powder O increasing the concentration of calcium chloride decreasing the amount of hydrochloric acid O decreasing the concentration of hydrochloric acid Lit AM
NA van wwwwwwww 1. For the reaction, 2 NO (g) + 2 H₂ (g) = following equilibrium concentrations: [NO]= 8.1 x 10-³ M [N2] = 0.053 M N₂ (g) + 2 H₂O (g), calculate Keq given the [H₂] = 4.1 x 10-5 M [H₂O]= 2.9 x 10-³ M 2. Given the reaction, UO2 (g) + 4 HF (g) = UF4 (g) + 2 H₂O (g), predict the effect each of the following will have on the equilibrium of the reaction (shift to the reactant side, the product side, or no shift). a. Uranium dioxide (UO2) is added. c. Water vapor is removed. b. Hydrogen fluoride (HF) reacts with the walls of the reaction vessel. - 3. At a certain temperature, Keq = 150 for the reaction being studied in today's lab. Use Equation (3) to calculate the concentrations of Fe³+ and SCN in a solution that has an equilibrium FeSCN2+ concentration of 4.5 x 105 M. Assume the equilibrium concentrations of Fe³+ and SCN are equal.
Consider the following reaction where Ke = 1.80 x 10-4 at 298 K. NH4HS(s) ⇒ NH3 (9) + H₂S(9) A reaction mixture was found to contain 0.0584 moles of NH4HS(s), 0.00833 moles of NH3(g), and 0.0134 moles of H₂S(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe, equals The reaction O must run in the forward direction to reach equilibrium. O must run in the reverse direction to reach equilibrium. O is at equilibrium.
The reaction Na₂SO4 10H₂O → Na₂SO4(s) + 10H₂O(g) has a K₂ R = 0.08206 Latm mol K Select one: O a. 2.02 x 10-14 O b. 3.08 x 10 12 O c. 7.93 x 10-26 O d. 2.23 x 10 13 O e. none of the following 5.38 x 10 12 at 21.3°C What is its Ke?
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