![The decomposition of N2Os(8) to NO2() and O2(g) obeys first-order kinetics. Assuming the form of the rate law is: A[N,Os] Rat](http://img.homeworklib.com/questions/c635fd30-ed09-11ea-aa5e-89f06a3028c0.png?x-oss-process=image/resize,w_560)
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The decomposition of N2Os(8) to NO2() and O2(g) obeys first-order kinetics. Assuming...
9,10,11 9. Consider the decomposition reaction of N2Os. 2 N203(g) → 4NO2(g) + O2(g) follows the...
9,10,11
9. Consider the decomposition reaction of N2Os. 2 N203(g) → 4NO2(g) + O2(g) follows the first order kinetics with rate constant of 4.8 x 10's. (a) if the initial 165 x 10-2M what is the concentration at 825 s? (b) How long it will take for concentration is 1.65 x 10-2M what is the concentrat the concentration of N2Os to decrease to 1.00 x 10-2M? t 10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows...
6. (a) The rate constant for the first-order decomposition of N2Os in the reaction, 2 N2Os(g)-4...
6. (a) The rate constant for the first-order decomposition of N2Os in the reaction, 2 N2Os(g)-4 NO(g)+0.(g), k-3x10-s at 25°C. What is the half-life of N20s? What will be the pressure, initially 500 bar, at 10 min after initiation of the reaction? (b) Knowing the activation energy of the above reaction is 100 kJ mor', calculate the required reaction temperature at which the reaction rate is doubled. (c) What is the conversion efficiency of N20s at 1 bar and 25...
Be sure to answer all parts. The gas-phase decomposition of peroxyacetyl nitrate (PAN) obeys first-order kinetics:...
Be sure to answer all parts. The gas-phase decomposition of peroxyacetyl nitrate (PAN) obeys first-order kinetics: CH3COOONO2 + CH3C000 + NO2 with a rate constant of 4.9 x 10-45-1. Calculate the rate of decomposition (in M/s) if the concentration of PAN is 0.35 ppm by volume. Assume STP conditions. rate= x 100 M/s (Enter your answer in scientific notation.)
14.44 The first-order rate constant for the decomposition of N205, 2N205(g)-→ 4 NO2(g) + O2(g), at...
14.44 The first-order rate constant for the decomposition of N205, 2N205(g)-→ 4 NO2(g) + O2(g), at 70°C is 6.82 × 10-3 s-1. Suppose we start with 0.250 mol of N205(g) 1S in a volume of 2.0 L. (a) How many moles of N2O5 will re- main after 10.0 min? (b) How many minutes will it take for the quantity of N205 to drop to 0.100 mol? (c) What is the half-life, in minutes, of N2Os at 70 °C?
The first-order rate constant for the gas-phase decomposition of N2O5 to NO2 and O2 at 65oC...
The first-order rate constant for the gas-phase decomposition
of N2O5 to NO2 and O2 at 65oC is 4.87 x 10-3/sec.
(a) If a chemist starts with 0.550 moles of N2O5 in a 500.0 ml
container, how many moles
of N2O5 will remain after 18.0 minutes? (b) How long will it
take for the quantity of N2O5 to drop to 0.0550 moles?
14. The first-order rate constant for the gas-phase decomposition of N205 to NO2 and O2 at 65℃ is 4.87...
The decomposition of phosphine, PH3, follows first-order kinetics: 4 PH3(g) → P4(g) + 6 H2(g) Calculate...
The decomposition of phosphine, PH3, follows first-order kinetics: 4 PH3(g) → P4(g) + 6 H2(g) Calculate the activation energy, Eq, in kJ/mol for the reaction, given that the rate constant k (at 25 °C) = 0.00852 s 1 and k (at 50 °C) = 0.756 s 1. 231 kJ/mol 144 kJ/mol O 56.5 kJ/mol О 99.3 kJ/mol O 111 kJ/mol
First order Trendline for Ina R2 = 0.997 Ina 0 -1 -2 10 8 6 2...
First order Trendline for Ina R2 = 0.997 Ina 0 -1 -2 10 8 6 2 Time (hours) n (A) M Lecure notes Po.3 5 pts each 7. In lecture, real experimental data was presented for the decomposition reaction wherein N2Os decomposed to NO2 and O2 at 30C. Use the data provided to answer the following three questions a) Assume that the order of the reaction with respect to N:Os is either 1 What is the order? Support your contention...
6) The rate constant for the first-order decomposition of N2O5 in the reaction 2N2O5(g) → 4NO2(g)...
6) The rate constant for the first-order decomposition of N2O5 in the reaction 2N2O5(g) → 4NO2(g) + O2(g) is k=3.38 x 10-5 s-1 at 25°C. What is the half-life of N2O5? What will be the total pressure, initially 88.3 kPa for the pure N2O5 vapour, (a) 10 s, (b) 10 minutes after initiation of the reaction?
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is...
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is reported in units of sl. What is the overall order of the reaction? 2) The rate law for a reaction was reported as rate=k[A] [B][C] with molar concentrations in moles per cubic decimetre and time in seconds. What are the units of k? 3) The rate constant for the pseudo first-order acid- catalysed hydrolysis of glucose is 4.07' 10-s. Calculate the half-life for the...
please 6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall...
please
6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: O(g) + O(g) 20(8): rate-k[O][NO] Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: H:Os(aq) + (aq) → H2O(1) Ol(aq) --- -slow H2O2(aq) + Ol'(aq) → H2O(1) + O2(g) + l'(aq) ------fast What is:...
9,10,11
9. Consider the decomposition reaction of N2Os. 2 N203(g) → 4NO2(g) + O2(g) follows the first order kinetics with rate constant of 4.8 x 10's. (a) if the initial 165 x 10-2M what is the concentration at 825 s? (b) How long it will take for concentration is 1.65 x 10-2M what is the concentrat the concentration of N2Os to decrease to 1.00 x 10-2M? t 10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows...
6. (a) The rate constant for the first-order decomposition of N2Os in the reaction, 2 N2Os(g)-4 NO(g)+0.(g), k-3x10-s at 25°C. What is the half-life of N20s? What will be the pressure, initially 500 bar, at 10 min after initiation of the reaction? (b) Knowing the activation energy of the above reaction is 100 kJ mor', calculate the required reaction temperature at which the reaction rate is doubled. (c) What is the conversion efficiency of N20s at 1 bar and 25...
Be sure to answer all parts. The gas-phase decomposition of peroxyacetyl nitrate (PAN) obeys first-order kinetics: CH3COOONO2 + CH3C000 + NO2 with a rate constant of 4.9 x 10-45-1. Calculate the rate of decomposition (in M/s) if the concentration of PAN is 0.35 ppm by volume. Assume STP conditions. rate= x 100 M/s (Enter your answer in scientific notation.)
14.44 The first-order rate constant for the decomposition of N205, 2N205(g)-→ 4 NO2(g) + O2(g), at 70°C is 6.82 × 10-3 s-1. Suppose we start with 0.250 mol of N205(g) 1S in a volume of 2.0 L. (a) How many moles of N2O5 will re- main after 10.0 min? (b) How many minutes will it take for the quantity of N205 to drop to 0.100 mol? (c) What is the half-life, in minutes, of N2Os at 70 °C?
The first-order rate constant for the gas-phase decomposition
of N2O5 to NO2 and O2 at 65oC is 4.87 x 10-3/sec.
(a) If a chemist starts with 0.550 moles of N2O5 in a 500.0 ml
container, how many moles
of N2O5 will remain after 18.0 minutes? (b) How long will it
take for the quantity of N2O5 to drop to 0.0550 moles?
14. The first-order rate constant for the gas-phase decomposition of N205 to NO2 and O2 at 65℃ is 4.87...
The decomposition of phosphine, PH3, follows first-order kinetics: 4 PH3(g) → P4(g) + 6 H2(g) Calculate the activation energy, Eq, in kJ/mol for the reaction, given that the rate constant k (at 25 °C) = 0.00852 s 1 and k (at 50 °C) = 0.756 s 1. 231 kJ/mol 144 kJ/mol O 56.5 kJ/mol О 99.3 kJ/mol O 111 kJ/mol
First order Trendline for Ina R2 = 0.997 Ina 0 -1 -2 10 8 6 2 Time (hours) n (A) M Lecure notes Po.3 5 pts each 7. In lecture, real experimental data was presented for the decomposition reaction wherein N2Os decomposed to NO2 and O2 at 30C. Use the data provided to answer the following three questions a) Assume that the order of the reaction with respect to N:Os is either 1 What is the order? Support your contention...
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is reported in units of sl. What is the overall order of the reaction? 2) The rate law for a reaction was reported as rate=k[A] [B][C] with molar concentrations in moles per cubic decimetre and time in seconds. What are the units of k? 3) The rate constant for the pseudo first-order acid- catalysed hydrolysis of glucose is 4.07' 10-s. Calculate the half-life for the...
please
6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: O(g) + O(g) 20(8): rate-k[O][NO] Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: H:Os(aq) + (aq) → H2O(1) Ol(aq) --- -slow H2O2(aq) + Ol'(aq) → H2O(1) + O2(g) + l'(aq) ------fast What is:...
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