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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?
(b) If you start with 0.052 M I2 at this temperature, how much will remain after 5.16 s assuming that the iodine atoms do not recombine to form I2?
According to the Bronsted-Lowry definition, which chemical in the following reaction is the acid? CO32- + H2O -> OH- + HCO3
Explain qualitatively how the following would change the calculated surface concentration of SO2 assuming a gaussian plume from a smoke stack that follows the gaussian equation for the concentration of SO2
Important information about Organic Chemistry, The most reasonable formula for a compound demonstrating M+ =101 with a minor M+1 peak is
Give the electron-domain and molecular geometries for the following molecules and ions (enter the appropriate number from thefollowing list).
A sample of air contains 78.08 % N2, 20.94% O2, 0.05 %CO2, 0.93% Ar by volume. a) How many molecules of each gas present in 1.00 L sample at 25 C and 1.00 atm. b)What is the partial pressure of each gas?
Explain why the Rf values changed when the eluant was changed from 100% petroleum ether to a 95:5 mixture of petroleum ether-ethyl acetate. Why UV light is not a useful visualization technique in every circumstances?
Naturally occuring chlorine has two isotopes, Cl-35, which has an atomic mass of 34.969 amu and Cl-37. If the average atomic mass of chlorine is 35.46 amu and its natural abundance is 75.53%
The next most abundent isotope is 26Mg, relative atomic mass 25.98259. The third Isotope is 25Mg whose natural abundance is in the ratio of 0.9083 to that of 26Mg. What is the relative atomic mass of 25Mg?
How many grams of O2 will be required to completely react with 2.43 grams of Mg metal ribbon to produce MgO.
Compute the number of moles - As we know many volatile substances are present in Earth's atmosphere in trace amounts.
a sample of nitrogen gas occupies 1.55 l at 27.0c and 1.00atm. what will be the volume be at -100.0 C and the same pressure
Calculate the equilibrium constant at 0c and at 50c(assuming enthalpies of formation are independent of temp)
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