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1. The rate constant for the following equation is 0.0391 M-1 · s-1. We start with 0.238 mol C2F4 in a 4.00-liter container, with no C4F8 initially present. 2C2F4 ?C4F8. What will be the concentration of C2F4 after 2.00 hours.
2. What will be the concentration of C4F8 after 2.00 hours? Note that this is the PRODUCT of the reaction.
Which of the seven cations will be the hardest to detect (same anions as above), Why do you think this? If two or more are possible explain why.
If 0.345 moles are produced during a reaction and collected at a temperature of 294K and pressire of .981 atm what volume will the gas occupy?
what wavelength of light in nm is absorbed by a ground state hydrogen atom could cause an electron to transition to n=3
Explain why water boils at a lower temperature (
Calculate the solubility of MnOH2 in grams per liter when buffered at pH=7.0 and pH=9.8 and pH=11.6
a compound is found to contain 39.12 carbon 8.772 hydrogen and 52.11 oxygen by weight. what is the empirical
A cylindrical vessel with rigid adiabatic walls is separated into two parts by a frictionless adiabatic adiabatic piston. Each part contains 50.0L of an ideal monatomic gas with Cv = 3R/2. Initially, Ti = 325K and Pi = 2.50x10^5 Pa in each part.
Separat the components of a water-insoluble mixture of barium sulfate (BaSO4) and nickel (ii) carbonate (NiCO3). Chemicals provied to aid in the separation and recovery of the 2 component mixturee are HCl(aq) and K2CO3(aq)
Using the isothermal transformation diagram for an iron-carbon alloy of eutectoid composition, specify the nature of the final microstructure (in terms of microconstituents present and approximate percentages
Describe the difference between the following and list any particular advantage possessed by one over the other a)filters and monochromators as wavelength selectors
Calculate the heats of combustion for the following reactions from the standard enthalpies of formations listed in appendix 3: (a) 2H2(g) + O2(g) = 2H2O(l) (b) 2C2H2(g) + 5O2(g) = 4CO2(g) + 2H2O(l)
If the heat of combustion for a specific compound is -1100.0 kJ/mol and its molar mass is 75.49 g/mol, how many grams of this compound must you burn to release 390.70 kJ of heat
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