The decomposition of N2O5 in carbon tetrachloride proceeds as follows: 2N2O5→4NO2+O2 The rate law is first...
The decomposition of N2O5 in carbon tetrachloride proceeds as follows:
2N2O5→4NO2+O2 The rate law is first order in N2O5. At 64*C the rate constant is 4.82 ×10^−3s^−1
The rate law is 4.82x10-3s-1 [N2O5]
The rate of rxn when [N2O5]=2.40x10^-2 M is 1.16x10^-4 M/s
What happens to the rate when the concentration of N2O5 is doubled? What about halved?
The answers are NOT 9.64x10^-3 and 2.41x10^-3 M/s
Homework Answers
![a) if conc concentrati on of N2Ojis doubled rate of reaction(i)-1. 16x 10.4M/s conc [N205]C)-2.40x 102M if C 2x2.40x102M then](http://img.homeworklib.com/questions/c92e14d0-8b3e-11eb-82b3-bfece2b23a2a.png?x-oss-process=image/resize,w_560)
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The decomposition of N2O5 in carbon tetrachloride proceeds as
follows:
2N2O5→4NO2+O2 The
rate law is first...
The decomposition of N2O5 in carbon tetrachloride proceeds as follows: What is the rate of reaction...
The decomposition of N2O5 in carbon tetrachloride proceeds as follows: What is the rate of reaction when N205] = 0.0270? Express the rate in molarity per second to three significant figures. 2N2O3 + 4NO2 + O2 The rate law is first order in N2O5. At 64 °C the rate constant is 4.82 x 10-3 3-1 IV AP R O 2 ? You may want to reference (Pages 576 - 581) Section 14.3 while completing this problem. rate = M /S...
The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction: 2N2O5 (soln) →...
The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction: 2N2O5 (soln) → 4NO2 (soln) + O2 (soln) The reaction is first order and has a rate constant of 4.82 x 10-3 s-1 at 64 oC. The reaction is initiated with 0.058 mol in a 1.25 L vessel. What is the half-life of the reaction?
The decomposition of N2O5 can be described by the equation 2n2O5>4NO2+O2 Given these data for ...
The decomposition of N2O5 can be described by the equation 2n2O5>4NO2+O2 Given these data for the reaction at 45�C in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval. t(s) [N2O5] 0 2.04 135 1.87 536 1.46 795 1.24 Reaction rate from 0-135 ?? Reaction rate from 135-536 ?? Reaction rate from 536-795 ??
The decomposition of N2O5 can be described by the equation 2N2O5(soln)⟶4NO2(soln)+O2(g) Consider the data in the...
The decomposition of N2O5 can be described by the equation 2N2O5(soln)⟶4NO2(soln)+O2(g) Consider the data in the table for the reaction at 45 ∘C in carbon tetrachloride solution. ? (?) [N2O5] (?) 0 1.934 225 1.679 556 1.363 795 1.173 Given the data, calculate the average rate of reaction for each successive time interval. A) What is the average rate of reaction for the time interval from 0 s0 s to 225 s? B) What is the average rate of reaction...
The decomposition of N2O5 is described by the following equation. 2N2O5(g) → 4NO2(g) + O2(g) If...
The decomposition of N2O5 is described by the following equation. 2N2O5(g) → 4NO2(g) + O2(g) If the rate constant is 2.50 × 10−4 s−1, what is the half-life of this reaction?
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?
The decomposition of N2O5 18.3 2N2O5 4NO2+O2 is studied by measuring the concentration of oxygen as...
The decomposition of N2O5 18.3 2N2O5 4NO2+O2 is studied by measuring the concentration of oxygen as a func- tion of time, and it is found that OlP dt (1.5 x 10sN2O5] = at constant temperature and pressure. Under these conditions the reaction goes to completion to the right. What is the half- life of the reaction under these conditions?
The decomposition of N2O5 can be described by the equation. 2N2O5
The decomposition of N2O5 can be described by the equation. 2N2O5 (soln) ---> 4NO2 (soln) + 2 (g) Given this data for the reaction at 45 degrees C in carbon tetrachloride solution, calculate the average rate for each successive time interval. t(s) [N2O5] (M) 0 2.10 195 1.86 556 1.48 825 1.25 Interval: 0 s to 195 s Reaction rate= _____M/s 195 s to 556 s Reaction rate= _____M/s 556 s to 825 s Reaction rate= _____M/s
The decomposition of N2O5N2O5 can be described by the equation 2N2O5(soln)⟶4NO2(soln)+O2(g) Consider the data in the...
The decomposition of N2O5N2O5 can be described by the equation 2N2O5(soln)⟶4NO2(soln)+O2(g) Consider the data in the table for the reaction at 45 ∘C45 ∘C in carbon tetrachloride solution. ? (?)t (s) [N2O5] (?)[N2O5] (M) 0 2.540 205 2.233 476 1.883 765 1.570 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time interval from 0 s0 s to 205 s? average rate of reaction: M/sM/s What...
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Suppose...
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Suppose we start with 2.40×10−2 mol of N2O5(g) in a volume of 2.1 L. a) How many moles of N2O5 will remain after 7.0 min? b) How many minutes will it take for the quantity of N2O5 to drop to 1.6×10−2 mol?
The decomposition of N2O5 in carbon tetrachloride proceeds as follows: What is the rate of reaction when N205] = 0.0270? Express the rate in molarity per second to three significant figures. 2N2O3 + 4NO2 + O2 The rate law is first order in N2O5. At 64 °C the rate constant is 4.82 x 10-3 3-1 IV AP R O 2 ? You may want to reference (Pages 576 - 581) Section 14.3 while completing this problem. rate = M /S...
The decomposition of N2O5 18.3 2N2O5 4NO2+O2 is studied by measuring the concentration of oxygen as a func- tion of time, and it is found that OlP dt (1.5 x 10sN2O5] = at constant temperature and pressure. Under these conditions the reaction goes to completion to the right. What is the half- life of the reaction under these conditions?
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