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5. A student is asked to find the rate constant for a first-order reaction, given that...
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 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 rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate =...
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...
the first order decomposition of N2O5 at 328 K has a rate constant of 1.70x10^-3 s^-1....
the first order decomposition of N2O5 at 328 K has a rate constant of 1.70x10^-3 s^-1. if the initial concentration of N2O5 is 2.88 M, what is the concentration of N2O5 after 12.5 minutes?
The rate constant for the first-order decomposition of N2O5 is 2.81×10−2 s−1 at 20∘C. If the...
The rate constant for the first-order decomposition of N2O5 is 2.81×10−2 s−1 at 20∘C. If the initial concentration of N2O5 is 2.50 M, what is the [N2O5] after 100 seconds?
For a first-order reaction, the half-life is constant. It depends only on the rate constant k...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant concentration. It is expressed as 0.693 - 1/2K For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as 1/2 k(Alo Part A A certain first-order reaction (A>products) has a rate constant of 9.60x10 s-1 at45 C. How many minutes does it take for the concentration of the...
A decomposition reaction in first order in A. If the rate constant of the reaction is...
A decomposition reaction in first order in A. If the rate constant of the reaction is 3.85 x 10-2s-1, how long will it take for 68% of the material to decompose?
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...
The first-order rate constant for the gas-phase decomposition of dimethyl ether, (CH3)20 → CH4 + H2...
The first-order rate constant for the gas-phase decomposition of dimethyl ether, (CH3)20 → CH4 + H2 + CO is 3.2 x 10-4 5-1 at 450°C. The reaction is carried out in a constant-volume container. Initially, only dimethyl ether is present, and the pressure is 0.343 atm. What is the pressure of the system after 8.1 min? Assume ideal-gas behavior. 49) 0.29 x 0.44 atm
The following reaction is first order in N2O5N2O5: N2O5(g)→NO3(g)+NO2(g)N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at...
The following reaction is first order in N2O5N2O5: N2O5(g)→NO3(g)+NO2(g)N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s/s. Part A Calculate the rate of the reaction when [N2O5]=[N2O5]= 5.1×10−2 MM. Express your answer using two significant figures. rate= ______ M/s Part B What would the rate of the reaction be at the same concentration as in Part A if the reaction were second order? (Assume the same numerical value for the rate constant with the appropriate units.)...
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...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant concentration. It is expressed as 0.693 - 1/2K For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as 1/2 k(Alo Part A A certain first-order reaction (A>products) has a rate constant of 9.60x10 s-1 at45 C. How many minutes does it take for the concentration of the...
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...
The first-order rate constant for the gas-phase decomposition of dimethyl ether, (CH3)20 → CH4 + H2 + CO is 3.2 x 10-4 5-1 at 450°C. The reaction is carried out in a constant-volume container. Initially, only dimethyl ether is present, and the pressure is 0.343 atm. What is the pressure of the system after 8.1 min? Assume ideal-gas behavior. 49) 0.29 x 0.44 atm
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