![11. The rate of decomposition of N203(g) to NO2(g) and NO(g) is followed by measuring [N02] at different times. The following](http://img.homeworklib.com/images/044cdea4-d015-4ddc-827f-66d4a7478cde.png?x-oss-process=image/resize,w_560)
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11. The rate of decomposition of N203(g) to NO2(g) and NO(g) is followed by measuring [N02] at di...
The rate of decomposition of N2O3(g)N2O3(g) to NO2(g)NO2(g) and NO(g)NO(g) is followed by measuring [NO2][NO2] at...
The rate of decomposition of N2O3(g)N2O3(g) to NO2(g)NO2(g) and NO(g)NO(g) is followed by measuring [NO2][NO2] at different times. The following data are obtained. [NO2](mol/L)[NO2](mol/L) 0 0.193 0.316 0.427 0.784 t(s)t(s) 0 884 1610 2460 50,000
please show steps so I can understand 2. Consider the decomposition of N,O, into NO, and...
please show steps so I can understand
2. Consider the decomposition of N,O, into NO, and NO. a. Write the balanced reaction equation for this decomposition. NO NO₂ + No. b. Write the expression for the rate of the reaction with respect to i. the reactant, N,O, - AN₂O3 At ii. the product NO ΔNOz + iii. the product NO ANO A+ c. The rate of decomposition was followed by measuring (NO) at different times. The data obtained is shown...
The rate of decomposition of N 2 O 3 (g) to NO 2 (g) and NO(g)...
The rate of decomposition of N 2 O 3 (g) to NO 2 (g) and NO(g) is followed by measuring [NO 2 ] at different times. The following data are obtained (10 pts): The reaction follows a first-order rate law. Calculate the rate constant. Assume that after 50,000 s all N 2 O 3 (g) had decomposed.
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 decomposition of NO2 was followed as a function of time; two different plots of the...
The decomposition of NO2 was followed as a function of time; two different plots of the data are shown here. Part A 400 Determine the order and rate constant for the reaction. O second order; 0.77 M-1.5-1 IONI O second order; 1.3 M-1.5-1 zero order; 0.0043 M/s O O zero order; 230 M/s 100 0 300 Submit 400 Request Answer 200 Time (s) 0,012 Provide Feedback 0,01 0,008 [NO2) 0.006 0,004 0.002 0 100 300 400 200 Time (s)
Example: The decomposition of NO2 at a moderately high temperature (between 300-400°C) +O2(g) 2NO(g) 2NO2( At 330...
Example: The decomposition of NO2 at a moderately high temperature (between 300-400°C) +O2(g) 2NO(g) 2NO2( At 330°C the rate constant for the decomposition of NO2 is 0.775 L/(mol sec) Suppose the initi concentration is 0.0030 mol/L. What is the concentration of NO2 after 645 s?
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?
Decomposition of nitrogen dioxide dimer N2O4 is described by the reaction: N2O4(g) = 2NO2(g) Concentration of...
Decomposition of nitrogen dioxide dimer N2O4 is described by the reaction: N2O4(g) = 2NO2(g) Concentration of N2O4 became 2 times less after 2,5⋅103 s. You have to calculate: a) the value of rate constant k of the reaction; b) the value of equilibrium constant Kp. You are given the value of standard Gibb’s energy of formation Goform: substance Goform, kJ/mol NO2(g) 51.6 N2O4(g) 98.4
2) 20 points in the lab you studied the decomposition of peroxide in ACIDIC solution If...
2) 20 points in the lab you studied the decomposition of peroxide in ACIDIC solution If the reaction is run under BASIC conditions a different result is obtained. 2 H2O2(aq) + 2 H2O(l) + O2(g) The rate of reaction can be determined by measuring the rate at which the volume of O2 increases at a pressure of latm. Use the data below to determine the rate law including! the value of the rate constant, “rate =k [H2021 [ITY". Show your...
Question 6 (18 marks) (a) Given that the rate constant k for the first-order decomposition of...
Question 6 (18 marks) (a) Given that the rate constant k for the first-order decomposition of compound X is 2.65 x 10-9 s', calculate the percentage of compound X that has decomposed in the first 2250 seconds after the reaction begins. (4 marks) (b) Consider the first order reaction: W2 → 2 Y. If [W2]=0.8 M initially and 0.17 M after 160 seconds, what will [W2] be after 350 seconds? (4 marks) (c) Data for the reaction 3A + 5B...
please show steps so I can understand
2. Consider the decomposition of N,O, into NO, and NO. a. Write the balanced reaction equation for this decomposition. NO NO₂ + No. b. Write the expression for the rate of the reaction with respect to i. the reactant, N,O, - AN₂O3 At ii. the product NO ΔNOz + iii. the product NO ANO A+ c. The rate of decomposition was followed by measuring (NO) at different times. The data obtained is shown...
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 decomposition of NO2 was followed as a function of time; two different plots of the data are shown here. Part A 400 Determine the order and rate constant for the reaction. O second order; 0.77 M-1.5-1 IONI O second order; 1.3 M-1.5-1 zero order; 0.0043 M/s O O zero order; 230 M/s 100 0 300 Submit 400 Request Answer 200 Time (s) 0,012 Provide Feedback 0,01 0,008 [NO2) 0.006 0,004 0.002 0 100 300 400 200 Time (s)
Example: The decomposition of NO2 at a moderately high temperature (between 300-400°C) +O2(g) 2NO(g) 2NO2( At 330°C the rate constant for the decomposition of NO2 is 0.775 L/(mol sec) Suppose the initi concentration is 0.0030 mol/L. What is the concentration of NO2 after 645 s?
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?
2) 20 points in the lab you studied the decomposition of peroxide in ACIDIC solution If the reaction is run under BASIC conditions a different result is obtained. 2 H2O2(aq) + 2 H2O(l) + O2(g) The rate of reaction can be determined by measuring the rate at which the volume of O2 increases at a pressure of latm. Use the data below to determine the rate law including! the value of the rate constant, “rate =k [H2021 [ITY". Show your...
Question 6 (18 marks) (a) Given that the rate constant k for the first-order decomposition of compound X is 2.65 x 10-9 s', calculate the percentage of compound X that has decomposed in the first 2250 seconds after the reaction begins. (4 marks) (b) Consider the first order reaction: W2 → 2 Y. If [W2]=0.8 M initially and 0.17 M after 160 seconds, what will [W2] be after 350 seconds? (4 marks) (c) Data for the reaction 3A + 5B...
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