A compound dissociates into its elements at 625 K in a first order process with a rate constant of 0.063s-1.
If you start with a 0.26 M concentration of the compound at this temperature, what will the concentration be after 2.285s?
(Assume that the compound is not reformed once it dissociates.)
I am not sure how to solve it :(((( Please help me.
A compound dissociates into its elements at 625 K in a first order process with a...
Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s-1. (a) What is the half-life for this reaction? _______ s (b) If you start with 0.051 M I2 at this temperature, how much will remain after 5.30 s assuming that the iodine atoms do not recombine to form I2? _______ M
Molecular iodine, I2 (g), dissociates into iodine
atoms at 652 K, with a first order rate constant of 0.452
s-1.
a. What is the half life for this reaction?
[ Select ]
["1.53 s", "0.31 s", "0.079 s", "0.39 s"]
b. If you start with 0.35 M I2 at this temperature,
how long will it take for the concentration of I2 to
reach...
Question 24 4 pts Molecular iodine, 12 (g), dissociates into iodine atoms at 652 K, with a first order rate constant of 0.452 5-1. 12 (g) 21 a. What is the half life for this reaction? 1.53 s b. If you start with 0.35 M 12 at this temperature, how long will it take for the concentration of 12 to reach 0.12 M? [ Select]
Compound X is known to decompose by a first-order process. If the concentration of X drops from 2.15 M to 0.41 M after 32.6 hours, what is the half-life?
Compounds A and B are unstable and each decomposes by a first-order process. At 398 K, the rate constant for the decomposition of A is 3.6 X 10-5 s-1. Separate containers of A and B were prepared, with initial concentrations of 0.120 M A and 0.240 M B. After 5 hrs, it was found that the concentration of A was three times the concentration of B wwww What was the concentration of A after 5 hrs? 2) 1) What is...
The first-order decomposition of a compound has a rate constant of 3.2 * 10-35-1 if the initial concentration of the compound is 6.50 M, what is the concentration of the compound after 855 s?
Need help with Part B
KAssignment 16 Chap 14: Integrated Rate Law and Half Life Problem 14.42 - Enhanced - with Feedback 5 of 7 Review I Constants I Periodic Table Molecular iodine, I2 (g), dissociates into iodine atoms at 625 K with a first-order rate constant of What is the half-life for this reaction? -1 0.271 S Express the half-life in seconds to three significant figures. You may want to reference (Pages 582-587) Section 14.4 while completing this problem....
The first-order decomposition of a compound has a rate constant of 3.2 x 10-35-1. If the initial concentration of the compound is 6.50 M, what is the concentration of the compound after 855 s? O 0.15 M O 0.42M 0.94 M O 0.67 M 0.86 M
1. For a first order k = 9.09x10-3 1/s. If the initial concentration is 7.06 M calculate the concentration after 35.0 s. 2. How long does it take the initial concentration of 0.778 M reduce to 0.453 M when k for the first order reaction is 2.11x10-2 1/min.? 3. The rate constant for a reaction at 25.0 oC is 2.87x10 -2. What is the rate constant at 55.0 oC? E a= 20.5 kJ. 4. The decomposition of a substance is...
The decomposition of a compound follows a first order kinetics with a rate constant of 0.0432 s^-1 at 500 degrees C. 1) if the initial concentration of starting material was 0.0500 M, what is the concentration after 1.4 min? 2) how long (in mins)will it take for the concentration of starting material to decrease from 0.750 M to 0.000250 M? 3) how long (in min) will it take to convert 32 percent of the starting material?