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Problem 2) Experimentally, the reaction between compound A and iodine (l): A(aq) + 12(aq) - D(aq)...
2. Consider the reaction below between nitric oxide and hydrogen gas: 2 NO(g) + 2 H2(g)...
2. Consider the reaction below between nitric oxide and hydrogen gas: 2 NO(g) + 2 H2(g) - N2 + 2 H2009) Upon being studied experimentally, it has been determined that the rate law expression for this reaction is first order in Hz and second order in NO(g). With this information in mind, answer the following: [Tip: You can assume that the steady-state approximation is valid for any intermediate here.) a. As written, is the reaction above a valid mechanism? In...
Help?? Consider the following reaction: H_2(g) hydrogen + 2ICI(g) iodine chloride righarrow HCI(g) hydrogen chloride +...
Help??
Consider the following reaction: H_2(g) hydrogen + 2ICI(g) iodine chloride righarrow HCI(g) hydrogen chloride + 1_2(g) iodine The rate law for this reaction has been determined experimentally, and it is first order in both hydrogen gas and iodine chloride gas (second order overall). Propose a mechanism with a minimum of two steps which is consistent with the observed rate law, and indicate which of the steps is likety to be the rate-determining step in the mechanism.
The following reaction was studied experimentally at 25 °C. S2O82(aq) + 21'(ag) = 12(aq) + 2SO4...
The following reaction was studied experimentally at 25 °C. S2O82(aq) + 21'(ag) = 12(aq) + 2SO4 (aq) The reaction was found to be first order with respect to I and first order with respect to S208". A reaction was performed with [1] = 0.080 M and [S208²-] = 0.040 M. The initial rate of formation of 12 was found to be 1.25 x 10-M St. Provide an expression for the rate law for this reaction and determine the initial rate...
D18 Kinetics Review Sheets 8 H*(aq) + 4 Cl(aq) + MnO4 (aq) - 2 Cl(g) +...
D18 Kinetics Review Sheets 8 H*(aq) + 4 Cl(aq) + MnO4 (aq) - 2 Cl(g) + Mn(aq) + 4H2O(l) 1. Cl2 (9) can be generated in the laboratory by reacting potassium permanganate with an acidified solution of sodium chloride. The net-ionic equation for the reaction is given above. a. A 25.00 mL sample of 0.250 M NaCl reacts completely with excess KMnO.(aq). The Cl(a) produced is dried and stored in a sealed container. At 22°C the pressure of the Cl2(g)...
Question 5 and 6 Determine and report the rate law for the reaction of iodide and...
Question 5 and 6
Determine and report the rate law for the reaction of iodide and persul fate ions. Show all calculations and justifications. 2 3.Based on the rate law that you determined above, calculate the values and units of k for: a. the three initial rates experiments in Part A, b. the one initial rates experiment at a different temperature in Part B. 4Use your two experiments done at different temperatures to determine the activation energy Ea and the...
4. (22 pts) Consider the following exothermic reaction: H2O2 +2t + 2H' → 12 + 2H20...
4. (22 pts) Consider the following exothermic reaction: H2O2 +2t + 2H' → 12 + 2H20 Consider the following mechanism for this reaction H,02 + r-* Hol + OH' Hol + r- 12 + он. 20H 2H2 H20 slow fast fast a) What species are intermediates in the above mechanism? Any catalysts? b) Sketch an energy versus reaction progress plot for the three step mechanism and clearly label the rate determining step in your diagram. c) What rate law would...
There are compounds D and compound E that react to form compound F in a one-to-one...
There are compounds D and compound E that react to form compound F in a one-to-one molar ratio. Write this reaction What would you expect the rate law to be if this reaction was elementary? The experimentally determined rate law is second order with respect to E and zeroth order with respect to D. Propose a two-step mechanism that would explain this. Identify the relative rates of each elementary step in your above mechanism (slow or fast). Draw an energy...
Consider the following aqueous chemical reaction involving iodine (12), iodide (") and tri-iodidell3'); 12(aq) + l'(aq)...
Consider the following aqueous chemical reaction involving iodine (12), iodide (") and tri-iodidell3'); 12(aq) + l'(aq) → l'(aq) Kc = 0.1 To aboL beaker of pure water you add exactly 0.2 moles of both 12 and I (i.e. initial concentrations of 12 and I are both 0.2 M, and the initial concentration of \g* = 0.0 M). Utilize the ICE table method to calculate the concentration of lz once the system has established equilibrium 2.8x102 M 0.1M 2.0 M O...
The following reaction was studied in a differential reaction A+BC+ D It was experimentally obser...
it all the information I got
The following reaction was studied in a differential reaction A+BC+ D It was experimentally observed that the reaction appeared 2nd order at low concentrations of A, 0'h order at high A concentrations, and 1st order at intermediate A concentrations. Which of the following suggested rate laws is consistent with the experimental observations? (5 points) a) rate-ki(k2PA+ksPB) PB b) rate PA c) rate d) rate kPAPB .. rate _ e) 1+k//ksPB
The following reaction was...
3. For the reaction, H2O2 (aq) + 3 (aq) + 2 H (aq) → 2 H20...
3. For the reaction, H2O2 (aq) + 3 (aq) + 2 H (aq) → 2 H20 (1) + 1- (aq) Ot The rate law was experimentally determined to be Rate = k[H2O2][T] a. What is the reaction order in terms of H20,? b. What is the reaction order in terms of I? because et is nuoto c. What is the reaction order in terms of HT? O d. What is the overall reaction order of this reaction? 4. If a...
2. Consider the reaction below between nitric oxide and hydrogen gas: 2 NO(g) + 2 H2(g) - N2 + 2 H2009) Upon being studied experimentally, it has been determined that the rate law expression for this reaction is first order in Hz and second order in NO(g). With this information in mind, answer the following: [Tip: You can assume that the steady-state approximation is valid for any intermediate here.) a. As written, is the reaction above a valid mechanism? In...
Help??
Consider the following reaction: H_2(g) hydrogen + 2ICI(g) iodine chloride righarrow HCI(g) hydrogen chloride + 1_2(g) iodine The rate law for this reaction has been determined experimentally, and it is first order in both hydrogen gas and iodine chloride gas (second order overall). Propose a mechanism with a minimum of two steps which is consistent with the observed rate law, and indicate which of the steps is likety to be the rate-determining step in the mechanism.
The following reaction was studied experimentally at 25 °C. S2O82(aq) + 21'(ag) = 12(aq) + 2SO4 (aq) The reaction was found to be first order with respect to I and first order with respect to S208". A reaction was performed with [1] = 0.080 M and [S208²-] = 0.040 M. The initial rate of formation of 12 was found to be 1.25 x 10-M St. Provide an expression for the rate law for this reaction and determine the initial rate...
D18 Kinetics Review Sheets 8 H*(aq) + 4 Cl(aq) + MnO4 (aq) - 2 Cl(g) + Mn(aq) + 4H2O(l) 1. Cl2 (9) can be generated in the laboratory by reacting potassium permanganate with an acidified solution of sodium chloride. The net-ionic equation for the reaction is given above. a. A 25.00 mL sample of 0.250 M NaCl reacts completely with excess KMnO.(aq). The Cl(a) produced is dried and stored in a sealed container. At 22°C the pressure of the Cl2(g)...
Question 5 and 6
Determine and report the rate law for the reaction of iodide and persul fate ions. Show all calculations and justifications. 2 3.Based on the rate law that you determined above, calculate the values and units of k for: a. the three initial rates experiments in Part A, b. the one initial rates experiment at a different temperature in Part B. 4Use your two experiments done at different temperatures to determine the activation energy Ea and the...
4. (22 pts) Consider the following exothermic reaction: H2O2 +2t + 2H' → 12 + 2H20 Consider the following mechanism for this reaction H,02 + r-* Hol + OH' Hol + r- 12 + он. 20H 2H2 H20 slow fast fast a) What species are intermediates in the above mechanism? Any catalysts? b) Sketch an energy versus reaction progress plot for the three step mechanism and clearly label the rate determining step in your diagram. c) What rate law would...
There are compounds D and compound E that react to form compound F in a one-to-one molar ratio. Write this reaction What would you expect the rate law to be if this reaction was elementary? The experimentally determined rate law is second order with respect to E and zeroth order with respect to D. Propose a two-step mechanism that would explain this. Identify the relative rates of each elementary step in your above mechanism (slow or fast). Draw an energy...
Consider the following aqueous chemical reaction involving iodine (12), iodide (") and tri-iodidell3'); 12(aq) + l'(aq) → l'(aq) Kc = 0.1 To aboL beaker of pure water you add exactly 0.2 moles of both 12 and I (i.e. initial concentrations of 12 and I are both 0.2 M, and the initial concentration of \g* = 0.0 M). Utilize the ICE table method to calculate the concentration of lz once the system has established equilibrium 2.8x102 M 0.1M 2.0 M O...
it all the information I got
The following reaction was studied in a differential reaction A+BC+ D It was experimentally observed that the reaction appeared 2nd order at low concentrations of A, 0'h order at high A concentrations, and 1st order at intermediate A concentrations. Which of the following suggested rate laws is consistent with the experimental observations? (5 points) a) rate-ki(k2PA+ksPB) PB b) rate PA c) rate d) rate kPAPB .. rate _ e) 1+k//ksPB
The following reaction was...
3. For the reaction, H2O2 (aq) + 3 (aq) + 2 H (aq) → 2 H20 (1) + 1- (aq) Ot The rate law was experimentally determined to be Rate = k[H2O2][T] a. What is the reaction order in terms of H20,? b. What is the reaction order in terms of I? because et is nuoto c. What is the reaction order in terms of HT? O d. What is the overall reaction order of this reaction? 4. If a...
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