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A 0.7549g sample of a pure hydrocarbon burns in oxygen gas to produce 1.9061g of carbon dioxide and 0.3370g of water.
a.) calculate the individual masses of C, H, and O in the sample
b.) What is the empirical formula for the compound?
a sample of argon gas is at a pressure of 1.24x10^4 kpa and a temperature of 24c in a rigid 25-L tank. How many moles of argon does this tank contain?
Decomposition of KClO3 is sometimes used to prepare small amounts of O2 in the laboratory: 2KClO3(s) 2 KCl(s) + 3 O2(g). How many grams of O2 can be prepared from 4.50 g of KClO3?
An amount of 0.500 grams of NH4Cl was added to 50.0 mL of the solution in Problem 1 above. Use the Keq calculated from problem 1 to calculate the pH of this solution.
Suppose an additional gaseous component, e.g. helium, is pumped into the system, keeping the volume of the container fixed, until the final pressure is 100 atm. Assume that the helium does not dissolve in water but remains pure. Assume water is in..
Draw and name all dienes of molecular formula C5H8. When E and Z isomers are possible, draw and name each stereoisomer
Separation of acetone from water by using MIBK - How much MIBK must be used if the final acetone concentration in the water-rich phase is 5 wt%?
Assume you have a jar of pulverized rock to test. Create a detailed 4-step procedure describing how you expect to go about doing this.
How many independent linear combinations are possible for four 1s orbitals? (b) Draw pictures of the linear combinations of H1s orbitals for a hypothetical linear H4 molecule.
Estimate the value of the equilibrium constant at 610K for each of the following reactions. Delta Hf and S for BrCl is 14.6 kj/mol and 240.0 J/mol*K , respectively. Br2(g)+ Cl2(g) --> 2BrCl(g)
Given the reaction PCl5 goes to PCl3 and Cl2. Starting with PCl5, calculate the equilibrium mole fractions of all species at 500 kelvin and 1.00 bar
Calculate the wavelength of a photon emitted when 1x10^-27 g particle in a box of a length 6.0 Angstrom goes from n=5
the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.500 M. N2(g)+O2(g)2NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-established?
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