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6. (a) The rate constant for the first-order decomposition of N2Os in the reaction, 2 N2Os(g)-4...
The decomposition of N2Os in CCl is a first-order reaction. If 3.98 mg of N20s is...
The decomposition of N2Os in CCl is a first-order reaction. If 3.98 mg of N20s is present initially and 3.91 mg is present after 3.13 minutes at 53 °C, what is the value of the rate constant? Rate constant- min-1
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?
6 (a) N2Os decomposes in the gas phase by the reaction: 2 N2Os (g)4 NO2 (g)+02 (g) At 25°C, a sample of gaseous N2Os sh...
6 (a) N2Os decomposes in the gas phase by the reaction: 2 N2Os (g)4 NO2 (g)+02 (g) At 25°C, a sample of gaseous N2Os showed the following dependence of concentration on time: IN:Os(mmol dm Time/h C0 8.0 5 4.3 10 2.3 15 1.20 0.64 20 ( Determine the order of reaction by plotting an appropriate graph. [5 marks] [2 marks] (ii) Determine the rate constant for this reaction. (ii) Find the concentration of NO2 after 25 h. [2 marks]
6...
7) The rate constant for the reaction 2N2O5(g) 25°C 4NO2(g) +O2(g) is k = 3.38x10-5/s at...
7) The rate constant for the reaction 2N2O5(g) 25°C 4NO2(g) +O2(g) is k = 3.38x10-5/s at a) Enter the half-life of N20s in seconds. Use two significant figures and do not enter units b) Enter the total pressure in kPa 10 seconds after initiation of the reaction if initially there was 88.3kPa of pure N2O5 vapor. Use two significant figures and do not enter the units c) Enter the total pressure in kPa 10 minutes after initiation of the reaction...
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...
The rate constant for the first-order decomposition of N_2O_5 in the xeactron2 N_2O_5(g) rightarroe 4 NO_2(g)+O_2(g)...
The rate constant for the first-order decomposition of N_2O_5 in the xeactron2 N_2O_5(g) rightarroe 4 NO_2(g)+O_2(g) is k_I = 3.38 times 10^-5 s^-1 at 25 degree C. What is the half-life of N205? What will be the pressure, initially 500 Torr, after 50 20 min after initiation of the reaction?
The rate constant for the first-order decomposition of a compound A in the reaction 2A rightarrow...
The rate constant for the first-order decomposition of a compound A in the reaction 2A rightarrow P is k = 3.6 times 10^-7 s^-1 at 25 degree C. What is the half-life of A? What will be the pressure, initially 33 kPa, at 50s, 20 min after initiation of the reaction?
show work please thanks The decomposition of N2Os(8) to NO2() and O2(g) obeys first-order kinetics. Assuming...
show work please thanks
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] Rate k[N,2,3 ΔΙ where k = 3.4 x 10-55 at 25°C, what is the initial rate of reaction at 25°C where (N2Oslo - 4.1 x 102 3.4 x 10-6 mol/L's 1.4 x 10-6 mol/L's O 8.3 x 10-mol/L's 4.1 x 10-2 mol/L'S none of these
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?
* 100%- 6 (a) NOs decomposes in the gas phase by the reaction: 2 N2Os (g)...
* 100%- 6 (a) NOs decomposes in the gas phase by the reaction: 2 N2Os (g) 4 NO2 (9)+ 02 (9) At 25'C, a sample of gaseous N,O, showed the following dependence of concentration on time: IN2Os/(mmol dm-3) 8.0 4.3 2.3 1.20 0.64 Time/h 10 15 20 (0 Determine the order of reaction by plotting an appropriate graph. (i) Determine the rate constant for this reaction. () Find the concentration of NO2 after 25 h [5 marks] [2 marks] 12...
The decomposition of N2Os in CCl is a first-order reaction. If 3.98 mg of N20s is present initially and 3.91 mg is present after 3.13 minutes at 53 °C, what is the value of the rate constant? Rate constant- min-1
6 (a) N2Os decomposes in the gas phase by the reaction: 2 N2Os (g)4 NO2 (g)+02 (g) At 25°C, a sample of gaseous N2Os showed the following dependence of concentration on time: IN:Os(mmol dm Time/h C0 8.0 5 4.3 10 2.3 15 1.20 0.64 20 ( Determine the order of reaction by plotting an appropriate graph. [5 marks] [2 marks] (ii) Determine the rate constant for this reaction. (ii) Find the concentration of NO2 after 25 h. [2 marks]
6...
7) The rate constant for the reaction 2N2O5(g) 25°C 4NO2(g) +O2(g) is k = 3.38x10-5/s at a) Enter the half-life of N20s in seconds. Use two significant figures and do not enter units b) Enter the total pressure in kPa 10 seconds after initiation of the reaction if initially there was 88.3kPa of pure N2O5 vapor. Use two significant figures and do not enter the units c) Enter the total pressure in kPa 10 minutes after initiation of the reaction...
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...
The rate constant for the first-order decomposition of N_2O_5 in the xeactron2 N_2O_5(g) rightarroe 4 NO_2(g)+O_2(g) is k_I = 3.38 times 10^-5 s^-1 at 25 degree C. What is the half-life of N205? What will be the pressure, initially 500 Torr, after 50 20 min after initiation of the reaction?
The rate constant for the first-order decomposition of a compound A in the reaction 2A rightarrow P is k = 3.6 times 10^-7 s^-1 at 25 degree C. What is the half-life of A? What will be the pressure, initially 33 kPa, at 50s, 20 min after initiation of the reaction?
show work please thanks
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] Rate k[N,2,3 ΔΙ where k = 3.4 x 10-55 at 25°C, what is the initial rate of reaction at 25°C where (N2Oslo - 4.1 x 102 3.4 x 10-6 mol/L's 1.4 x 10-6 mol/L's O 8.3 x 10-mol/L's 4.1 x 10-2 mol/L'S none of these
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?
* 100%- 6 (a) NOs decomposes in the gas phase by the reaction: 2 N2Os (g) 4 NO2 (9)+ 02 (9) At 25'C, a sample of gaseous N,O, showed the following dependence of concentration on time: IN2Os/(mmol dm-3) 8.0 4.3 2.3 1.20 0.64 Time/h 10 15 20 (0 Determine the order of reaction by plotting an appropriate graph. (i) Determine the rate constant for this reaction. () Find the concentration of NO2 after 25 h [5 marks] [2 marks] 12...
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