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.
Homework Answers
11. The rate of decomposition of N203(g) to NO2(g) and NO(g) is followed by measuring [N02] at di...
11. The rate of decomposition of N203(g) to NO2(g) and NO(g) is followed by measuring [N02] at different times. The following data are obtained (10 pts) NO2l(mol/L) 0.193 0.316 0.427 0.784 t (s) 0 8841610 2460 50,000 The reaction follows a first-order rate law. Calculate the rate constant. Assume that after 50,000 s all N203(g) had decomposed.
11. The rate of decomposition of N203(g) to NO2(g) and NO(g) is followed by measuring [N02] at different times. The following data are...
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 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
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...
In a study of the decomposition of nitrosyl bromide at 10 °C NOBr—+NO+ Br2 the concentration...
In a study of the decomposition of nitrosyl bromide at 10 °C NOBr—+NO+ Br2 the concentration of NOBr was followed as a function of time. It was found that a graph of 1/[NOBr] versus time in seconds gave a straight line with a slope of 1.27 m?s and a y-intercept of 3.98 M? Based on this plot, the reaction is order in NOBr and the rate constant for the reaction is M?? In a study of the decomposition of hydrogen...
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 initial concentration of N 2 O 5 (g) in the first-order reaction 2 N 2...
The initial concentration of N 2 O 5 (g) in the first-order reaction 2 N 2 O 5 (g)→4 NO 2 (g)+ O 2 (g) is 0.372 mol/L . After 30 seconds, the concentration of N 2 O 5 (g) is 0.0744 mol/L . What is the rate constant for the reaction?
In a study of the decomposition of nitrous oxide at 565 °C N20(g) N2(g) + %...
In a study of the decomposition of nitrous oxide at 565 °C N20(g) N2(g) + % O2(g) the following data were obtained: IN,O].M 1.81 0.905 663 0.453 .99 103 seconds 1 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.8 concentration is 0.905 M is s and when the starting (2) The average A(1/[N,O]) / At from t=0 s to t = 663 s is The...
The following data are obtained for the decomposition of N,Og at a certain temperature: 2N205(9) -...
The following data are obtained for the decomposition of N,Og at a certain temperature: 2N205(9) - 4NO2(g) + O2(9) Time(s) N205 (atm) 0 2.40 200 2.13 400 1.88 600 1.67 800 1.48 Find the rate constant kobs for this first-order decomposition reaction. (Enter in sec-1) Submit Answer Tries 0/99
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...
11. The rate of decomposition of N203(g) to NO2(g) and NO(g) is followed by measuring [N02] at different times. The following data are obtained (10 pts) NO2l(mol/L) 0.193 0.316 0.427 0.784 t (s) 0 8841610 2460 50,000 The reaction follows a first-order rate law. Calculate the rate constant. Assume that after 50,000 s all N203(g) had decomposed.
11. The rate of decomposition of N203(g) to NO2(g) and NO(g) is followed by measuring [N02] at different times. The following data are...
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...
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...
In a study of the decomposition of nitrosyl bromide at 10 °C NOBr—+NO+ Br2 the concentration of NOBr was followed as a function of time. It was found that a graph of 1/[NOBr] versus time in seconds gave a straight line with a slope of 1.27 m?s and a y-intercept of 3.98 M? Based on this plot, the reaction is order in NOBr and the rate constant for the reaction is M?? In a study of the decomposition of hydrogen...
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?
In a study of the decomposition of nitrous oxide at 565 °C N20(g) N2(g) + % O2(g) the following data were obtained: IN,O].M 1.81 0.905 663 0.453 .99 103 seconds 1 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.8 concentration is 0.905 M is s and when the starting (2) The average A(1/[N,O]) / At from t=0 s to t = 663 s is The...
The following data are obtained for the decomposition of N,Og at a certain temperature: 2N205(9) - 4NO2(g) + O2(9) Time(s) N205 (atm) 0 2.40 200 2.13 400 1.88 600 1.67 800 1.48 Find the rate constant kobs for this first-order decomposition reaction. (Enter in sec-1) Submit Answer Tries 0/99
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...
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