A certain substance, initially present at 0.950 M decomposes
A certain substance, initially present at 0.950 M decomposes by first order kinetics with a rate constant of 1.25 × 10-2 mol L-1s-1 Calculate the time (in seconds) required for the system to reach a concentration of 0.352M.
Homework Answers
A certain substance, initially present at 0.500 M, decomposes by second-order kinetics with a rate constant...
A certain substance, initially present at 0.500 M, decomposes by second-order kinetics with a rate constant of 4.00 × 10-1 L/mol min. Calculate the time (in minutes) required for the system to reach a concentration of 0.116 M. ___ min?
A certain substance, initially at 0.10 M in solution, decomposes by second-order kinetics. If the rate...
A certain substance, initially at 0.10 M in solution, decomposes by second-order kinetics. If the rate constant for this process is 0.40 L/mol • min, how much time is required for the concentration to reach 0.020 M?
10 and 11 10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows...
10 and 11
10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows second order kinetics with a rate constant of 0.020 L mol-' s at a certain temperature. 2 NOCI (g) → 2 NO(g) + Cl2(g) If the initial concentration of NOCI in a closed reaction vessel is 0.050 M, what will be the concentration be after 30 minutes? 11. The reaction 2 NO2 (g) → 2 NO(g) + O2(g), is second order with respect to...
A gas decomposes to form O2 and two other products, in a first-order reaction, with rate...
A gas decomposes to form O2 and two other products, in a first-order reaction, with rate constant k = 6.95 x 10 –4/s at 40oC. If the initial gas concentration = 4.80 x 10 –2 mol/L, what is the concentration (M) after 250 seconds have passed?
At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.0569·M−1s−1: ClCH2CH2Cl(g)...
At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.0569·M−1s−1: ClCH2CH2Cl(g) → CH2CHCl(g) + HCl(g) Suppose a vessel contains ClCH2CH2Cl at a concentration of 0.730M. Calculate the concentration of ClCH2CH2Cl in the vessel 320. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. _ M
1. A reaction was shown to follow second-order kinetics. How much time is required for [A]...
1. A reaction was shown to follow second-order kinetics. How much time is required for [A] to change from 0.500 M to 0.160 M? (k = 0.456 M⁻¹ s⁻¹) 2. A substance decomposes with a rate constant of 9.05 × 10⁻⁴ s⁻¹. How long does it take for 16.0% of the substance to decompose? 3. How long will it take for the concentration of A to decrease from 0.500 M to 0.100 M in the first-order reaction A → B?...
Be sule to answer all parts Ethyl iodide (C2Hgl) decomposes at a certain temperature in the...
Be sule to answer all parts Ethyl iodide (C2Hgl) decomposes at a certain temperature in the gas phase according to first-order kinetics as follows: The rate constant for this reaction is k-228x 10-*s-1. Use it to fill in the missing values in the following table: Time (min) [C2H;I (M) 0.49 10 20 30 40 [C2Hsll1o min -0.392 [C2H51]20 min-10.365 I 2115130 min IC2Hs1l40 min 0.277
For the reaction 2NO2 + F2 2NO2F, the rate constant is 38M-1s-1. The reaction is first...
For the reaction 2NO2 + F2 2NO2F, the rate constant is 38M-1s-1. The reaction is first order in NO2 and first order in F2, being of the second order total. Calculate the concentration of NO2, F2, and NO2F present after 30.0 seconds, if initially 3.00 mol of NO2 are mixed. with 1.00 mol of F2 in a container of 400 dm3 at 27oC.
O KINETICS AND EQUILIBRIUM Using a second order integrated rato low to find concentration '. At...
O KINETICS AND EQUILIBRIUM Using a second order integrated rato low to find concentration '. At a certain temperature this reaction follows second-order kinetics with a rate constant of 13.1 M 250,() 250,()+0,6) Suppose a vessel contains so, at a concentration of 0.130 M. Calculate the concentration of SO, in the vessel 9.20 seconds later. You may assume no other reaction is important Round your answer to 2 significant digits. O KINETICS AND EQUILIRIUM Using the Arrhenius equation to calculate...
Part A The rate constant for a certain reaction is k = 7.60x10-35-?. If the initial...
Part A The rate constant for a certain reaction is k = 7.60x10-35-?. If the initial reactant concentration was 0.950 mol L-, what will the concentration be after 5.00 minutes? Express your answer with the appropriate units. View Available Hint(s) Value Units Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining Part B . If after 65.0 seconds the concentration has dropped to 1.50x10-2 A zero-order reaction has a constant rate of 4.50x10-mol L-8 mol L , what was...
10 and 11
10. Nitrosyl chloride, NOCI, decomposes slowly to NO and Cl2, the reaction follows second order kinetics with a rate constant of 0.020 L mol-' s at a certain temperature. 2 NOCI (g) → 2 NO(g) + Cl2(g) If the initial concentration of NOCI in a closed reaction vessel is 0.050 M, what will be the concentration be after 30 minutes? 11. The reaction 2 NO2 (g) → 2 NO(g) + O2(g), is second order with respect to...
Be sule to answer all parts Ethyl iodide (C2Hgl) decomposes at a certain temperature in the gas phase according to first-order kinetics as follows: The rate constant for this reaction is k-228x 10-*s-1. Use it to fill in the missing values in the following table: Time (min) [C2H;I (M) 0.49 10 20 30 40 [C2Hsll1o min -0.392 [C2H51]20 min-10.365 I 2115130 min IC2Hs1l40 min 0.277
O KINETICS AND EQUILIBRIUM Using a second order integrated rato low to find concentration '. At a certain temperature this reaction follows second-order kinetics with a rate constant of 13.1 M 250,() 250,()+0,6) Suppose a vessel contains so, at a concentration of 0.130 M. Calculate the concentration of SO, in the vessel 9.20 seconds later. You may assume no other reaction is important Round your answer to 2 significant digits. O KINETICS AND EQUILIRIUM Using the Arrhenius equation to calculate...
Part A The rate constant for a certain reaction is k = 7.60x10-35-?. If the initial reactant concentration was 0.950 mol L-, what will the concentration be after 5.00 minutes? Express your answer with the appropriate units. View Available Hint(s) Value Units Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining Part B . If after 65.0 seconds the concentration has dropped to 1.50x10-2 A zero-order reaction has a constant rate of 4.50x10-mol L-8 mol L , what was...
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