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The following data were obtained for the formation of nitrosyl bromide from nitrogen monoxide and bromine....
please help with these two questions The following data were obtained for the formation of nitrosyl...
please help with these two questions
The following data were obtained for the formation of nitrosyl bromide from nitrogen monoxide and bromine. Initial (NO) Initial (Bra) Initial rate of reaction Trial 1 0.025 M 0.040 M 1.2 m/s Trial 20.025 M 0.080 M 2.4 M/S Trial 3 0.025 M 0.120 M 3.6 M/s Trial 4 0.050 M 0.040 M 4.8 M/s Trial 5 0.075 M 0.040 M 10.8 Mis The rate law for this reaction would be: zero-order in NO...
The circles below represent the conversion of molecule A (closed circles) to B (open circles). •...
The circles below represent the conversion of molecule A (closed circles) to B (open circles). • = A O=B t=0 s t = 10 s t = 20 s What is the correct stoichiometry of the reaction shown in the diagram? O a AB O b. A2B O c. ЗА ЭВ Od 2A →B Cannot be determined from the information given. For the reaction N205 - NO3 + NO2 the observed rate law is rate = k[N205]. If-dN205/dt = 0.20...
8. Nitrosyl bromide (NOBr) decomposes to nitrogen oxide and bromine. Use the following data to determine...
8. Nitrosyl bromide (NOBr) decomposes to nitrogen oxide and bromine. Use the following data to determine the order of the decomposition reaction. time 6 12 18 24 INOBr] 0.0286 0.0253 0.0229 0.0208 0.0190 Ln NOB] -3.554 1 -3.677 -3.777 -3.873 -3.963 1/[NOBr] 35.0 39.5 43.7 48.1 52.6
Nitrogen dioxide reacts with carbon monoxide to produce nitric oxide as follows: NO2 (9) + CO...
Nitrogen dioxide reacts with carbon monoxide to produce nitric oxide as follows: NO2 (9) + CO (9) ► NO (9) + CO2 (g) The reaction is second order in NO2, zeroth order in CO and second order overall. How long (in hours) will it take for NO2 to decompose by 35.8% given the initial concentration was 0.43 M NO2 and CO was in excess. The rate constant for this reaction at 225°C is 2.08 x 10-4 L/mol/s. Report your answer...
Review Constants Periodic Tab Part A Butadiene (C4H6) reacts with itself to form a dimer with...
Review Constants Periodic Tab Part A Butadiene (C4H6) reacts with itself to form a dimer with the formula C8H12. The reaction is second order in C4H6. Assume the rate constant at a particular temperature is 4.0 x 10-2 M-18-1 and the initial concentration of C4H6 is 0.0180 M. What is its molarity after a reaction time of 1.30 h? Express your answer in moles per liter to two significant figures. Molarity = Submit Request Answer Part B What is the...
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...
need help with 2 and 3 2. A reaction D+B products is found to be zeroth...
need help with 2 and 3
2. A reaction D+B products is found to be zeroth order in B and second order in D. The Arrhenius equation is k = Ae ERT. In the Arrhenius equation, the units (the dimensions) of the quantity designated by A is/are: A) M/s B) 1/M's C) 1/s D) 1/ M S E) Cannot be determined from the information given 3. Consider the reaction N2(g) + O2(g) = 2NO(g), for which Kc = 0.10 at...
1) The following experimental data were obtained for a particular irreversible reaction at T = 25.0...
1) The following experimental data were obtained for a particular irreversible reaction at T = 25.0 °C. It is assumed that the reaction obeys a rate law of the form rate = - d[A]/dt = k [A]P [B]" (1.1) Trial [A]initial (mol/L) [B]initial (mol/L) (Rate) initial (mol/L•min) 0.00100 0.00100 0.00100 0.00100 0.00100 0.00200 0.00400 0.01000 2.6 x 10-8 1.2 x 10-7 3.9 x 10-7 2.4 x 10-6 0.00200 0.00400 0.01000 0.00200 0.00200 0.00200 1.5 x 10-7 1.1 x 107 1.6...
10 and 11 10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows...
10 and 11
10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows second order kinetics with a rate constant of 0.020 L mol-' s at a certain temperature. 2 NOCI (g) → 2 NO(g) + Cl2(g) If the initial concentration of NOCI in a closed reaction vessel is 0.050 M, what will be the concentration be after 30 minutes? 11. The reaction 2 NO2 (g) → 2 NO(g) + O2(g), is second order with respect to...
Consider the reaction A + B ? products From the following data obtained at a certain...
Consider the reaction A + B ? products From the following data obtained at a certain temperature, determine the rate law, the order of the reaction, and calculate the rate constant k. Experiment 1: [A] = 1.50 M; [B] = 1.50 M; Initial Rate = 3.20 x 10-1 M/s Experiment 2: [A] = 1.50 M; [B] = 2.50 M; Initial Rate = 3.20 x 10-1 M/s Experiment 3: [A] = 3.00 M; [B] = 1.50 M; Initial Rate = 6.40...
please help with these two questions
The following data were obtained for the formation of nitrosyl bromide from nitrogen monoxide and bromine. Initial (NO) Initial (Bra) Initial rate of reaction Trial 1 0.025 M 0.040 M 1.2 m/s Trial 20.025 M 0.080 M 2.4 M/S Trial 3 0.025 M 0.120 M 3.6 M/s Trial 4 0.050 M 0.040 M 4.8 M/s Trial 5 0.075 M 0.040 M 10.8 Mis The rate law for this reaction would be: zero-order in NO...
The circles below represent the conversion of molecule A (closed circles) to B (open circles). • = A O=B t=0 s t = 10 s t = 20 s What is the correct stoichiometry of the reaction shown in the diagram? O a AB O b. A2B O c. ЗА ЭВ Od 2A →B Cannot be determined from the information given. For the reaction N205 - NO3 + NO2 the observed rate law is rate = k[N205]. If-dN205/dt = 0.20...
8. Nitrosyl bromide (NOBr) decomposes to nitrogen oxide and bromine. Use the following data to determine the order of the decomposition reaction. time 6 12 18 24 INOBr] 0.0286 0.0253 0.0229 0.0208 0.0190 Ln NOB] -3.554 1 -3.677 -3.777 -3.873 -3.963 1/[NOBr] 35.0 39.5 43.7 48.1 52.6
Nitrogen dioxide reacts with carbon monoxide to produce nitric oxide as follows: NO2 (9) + CO (9) ► NO (9) + CO2 (g) The reaction is second order in NO2, zeroth order in CO and second order overall. How long (in hours) will it take for NO2 to decompose by 35.8% given the initial concentration was 0.43 M NO2 and CO was in excess. The rate constant for this reaction at 225°C is 2.08 x 10-4 L/mol/s. Report your answer...
Review Constants Periodic Tab Part A Butadiene (C4H6) reacts with itself to form a dimer with the formula C8H12. The reaction is second order in C4H6. Assume the rate constant at a particular temperature is 4.0 x 10-2 M-18-1 and the initial concentration of C4H6 is 0.0180 M. What is its molarity after a reaction time of 1.30 h? Express your answer in moles per liter to two significant figures. Molarity = Submit Request Answer Part B What is the...
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...
need help with 2 and 3
2. A reaction D+B products is found to be zeroth order in B and second order in D. The Arrhenius equation is k = Ae ERT. In the Arrhenius equation, the units (the dimensions) of the quantity designated by A is/are: A) M/s B) 1/M's C) 1/s D) 1/ M S E) Cannot be determined from the information given 3. Consider the reaction N2(g) + O2(g) = 2NO(g), for which Kc = 0.10 at...
1) The following experimental data were obtained for a particular irreversible reaction at T = 25.0 °C. It is assumed that the reaction obeys a rate law of the form rate = - d[A]/dt = k [A]P [B]" (1.1) Trial [A]initial (mol/L) [B]initial (mol/L) (Rate) initial (mol/L•min) 0.00100 0.00100 0.00100 0.00100 0.00100 0.00200 0.00400 0.01000 2.6 x 10-8 1.2 x 10-7 3.9 x 10-7 2.4 x 10-6 0.00200 0.00400 0.01000 0.00200 0.00200 0.00200 1.5 x 10-7 1.1 x 107 1.6...
10 and 11
10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows second order kinetics with a rate constant of 0.020 L mol-' s at a certain temperature. 2 NOCI (g) → 2 NO(g) + Cl2(g) If the initial concentration of NOCI in a closed reaction vessel is 0.050 M, what will be the concentration be after 30 minutes? 11. The reaction 2 NO2 (g) → 2 NO(g) + O2(g), is second order with respect to...
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