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The following data were collected for the reaction between hydrogen and nitric oxide at 700 C...
20. The reaction of nitric oxide (NO(g)) with a molecular hydrogen (H2(g)) results in the production...
20. The reaction of nitric oxide (NO(g)) with a molecular hydrogen (H2(g)) results in the production of molecular nitrogen and water as follows: 2NO(g) + 2H2(g) N20(g)+2H2O(g) According to the following proposed mechanism of this reaction 2NO(g) k-1 (fast equilibrium) N2O2(g) H2(g)+ N2O2(g) N2O(g)+2H20(g) Which of the following is TRUE A) The reaction rate of hydrogen decomposition is consistent with the observed 3rd order. The reaction rate of hydrogen decomposition is consistent with the observed 4th order. B) C) The...
1/ The Following data was obtained while observing a reaction between nitric oxide and hydrogen: F2(g)...
1/ The Following data was obtained while observing a reaction between nitric oxide and hydrogen: F2(g) + 2CLO2(g) -----> 2FCLO2(g) Experiment Initial(F2) Initial(CLO2) Initial rate (mol/L) (mol/L) (mol/L*s) 1/ 0.10 0.010 1.2 x 10^-3 2/ 0.10 0.040 4.8 x 10^-3 3/ 0.20 0.010 2.4 x 10^-3 A/ write the rate law for this reaction B/ calculate the rate constant for the reaction C/ what is the order of this reaction 2/ consider the reaction N2(g) + 3H2(g) ----> 2NH3(g). At...
23. Nitric oxide reacts with hydrogen at a measurable rate at 1 following equation: 2 NO...
23. Nitric oxide reacts with hydrogen at a measurable rate at 1 following equation: 2 NO + 2H2 → N2+ 2H2O The experimental rate law is Rate=k(NO]2[H] I concentration is measured in moles per liter, what are the units for the rate of 000 K according to the f time is measured in minutes and consumption of nitric oxide? A) L/(mol2 min) D) mof心.min). E) mol(L min). m012/(L2. min). mol/(L2. min) B) C) compound containing carbon and nitrogen has a...
1.The reaction of hydrogen and nitric oxide, shown below, is first order with respect to hydrogen...
1.The reaction of hydrogen and nitric oxide, shown below, is first order with respect to hydrogen and second order with respect to nitric oxide. Write the rate law for this reaction. (Rate expressions take the general form: rate = k . [A]a . [B]b.) 2 H2(g) + 2 NO(g) → N2(g) + 2 H2O(l) The rate law for a general reaction involving reactant A is given by the equation rate = k[A]2, 2. Where rate is the rate of the...
8. An instructor asked the class, "Can you substitute hydrogen in nitrous oxide booster in your...
8. An instructor asked the class, "Can you substitute hydrogen in nitrous oxide booster in your car engine, and if so what would be a representative reaction occurring in your car engine?" A half alert student thought he heard the instructor ask for the reaction between hydrogen and nitric oxide (instead of nitrous oxide NO2) and took off to perform the calculations. He assumed the reaction would be: 2H2 (g) + 2NO (g) → 2H,0 (g) + N2 (g) The...
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...
2) A proposed reaction mechanism for nitric oxide, NO, produced in hydrogen fueled jet engines 1s...
2) A proposed reaction mechanism for nitric oxide, NO, produced in hydrogen fueled jet engines 1s 2 NO(g) N202(g) N202(g) + H2(g) H20(g) +N20(g) N20(g) +H2(g) N2(g) + H20(g) fast slow fast a) Write a balanced equation for the overall chemical reaction (1/2 mark) b) Determine the theoretical rate law. (1 mark) c) Using the blank reaction progress diagram below sketch the energy profile of this exothermic reaction mechanism, labeling the positions of NO. H2,N 02, N2O, H2O, N2. (3...
18. The reaction of nitric oxide with hydrogen at 1280°C is: 2 NO (g) + 2...
18. The reaction of nitric oxide with hydrogen at 1280°C is: 2 NO (g) + 2 H2 (g) -> N2 (g) + 2 H20 (g) th From the following data determine the rate law and rate constant: Experiment [NO] [H] Initial Rate (M/s) 1 5.0 x 10-3 2.0 x 10-3 1.3 x 10-5 2 10.0 × 10-3 2.0 x 10-3 5.0 x 10-5 10.0 x 10-3 4.0 x 10-3 10.0 x 10-5 3 20 A. Rate = k [NO][H2] B....
The following initial rate data are for the reduction of nitric oxide with hydrogen: 2 NO...
The following initial rate data are for the reduction of nitric oxide with hydrogen: 2 NO + 2 H2N2 + 2 H2O Experiment [NO]o, M [H2]o, M Initial Rate, M s-1 1 0.367 0.448 8.93×10-2 2 0.734 0.448 0.357 3 0.367 0.896 0.179 4 0.734 0.896 0.714 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not...
step Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: elementary reaction...
step Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: elementary reaction rate constant NO(g) +0,() ► NO,()+(2) ky 2 NO(g) +0 (2) NOG) kz Suppose also , ekz. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates x 5 ?
20. The reaction of nitric oxide (NO(g)) with a molecular hydrogen (H2(g)) results in the production of molecular nitrogen and water as follows: 2NO(g) + 2H2(g) N20(g)+2H2O(g) According to the following proposed mechanism of this reaction 2NO(g) k-1 (fast equilibrium) N2O2(g) H2(g)+ N2O2(g) N2O(g)+2H20(g) Which of the following is TRUE A) The reaction rate of hydrogen decomposition is consistent with the observed 3rd order. The reaction rate of hydrogen decomposition is consistent with the observed 4th order. B) C) The...
23. Nitric oxide reacts with hydrogen at a measurable rate at 1 following equation: 2 NO + 2H2 → N2+ 2H2O The experimental rate law is Rate=k(NO]2[H] I concentration is measured in moles per liter, what are the units for the rate of 000 K according to the f time is measured in minutes and consumption of nitric oxide? A) L/(mol2 min) D) mof心.min). E) mol(L min). m012/(L2. min). mol/(L2. min) B) C) compound containing carbon and nitrogen has a...
8. An instructor asked the class, "Can you substitute hydrogen in nitrous oxide booster in your car engine, and if so what would be a representative reaction occurring in your car engine?" A half alert student thought he heard the instructor ask for the reaction between hydrogen and nitric oxide (instead of nitrous oxide NO2) and took off to perform the calculations. He assumed the reaction would be: 2H2 (g) + 2NO (g) → 2H,0 (g) + N2 (g) The...
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...
2) A proposed reaction mechanism for nitric oxide, NO, produced in hydrogen fueled jet engines 1s 2 NO(g) N202(g) N202(g) + H2(g) H20(g) +N20(g) N20(g) +H2(g) N2(g) + H20(g) fast slow fast a) Write a balanced equation for the overall chemical reaction (1/2 mark) b) Determine the theoretical rate law. (1 mark) c) Using the blank reaction progress diagram below sketch the energy profile of this exothermic reaction mechanism, labeling the positions of NO. H2,N 02, N2O, H2O, N2. (3...
18. The reaction of nitric oxide with hydrogen at 1280°C is: 2 NO (g) + 2 H2 (g) -> N2 (g) + 2 H20 (g) th From the following data determine the rate law and rate constant: Experiment [NO] [H] Initial Rate (M/s) 1 5.0 x 10-3 2.0 x 10-3 1.3 x 10-5 2 10.0 × 10-3 2.0 x 10-3 5.0 x 10-5 10.0 x 10-3 4.0 x 10-3 10.0 x 10-5 3 20 A. Rate = k [NO][H2] B....
step Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: elementary reaction rate constant NO(g) +0,() ► NO,()+(2) ky 2 NO(g) +0 (2) NOG) kz Suppose also , ekz. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates x 5 ?
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