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1) The four common isotopes of Sulfur have atomic masses of 32, 33, 34, and 35 amu, respectively. Draw valence diagrams of both atoms showing the electrons, neutrons and protons.
2) Write the electronic configuration in sublevels for the following atoms
i. 7N14
ii. 4Be9
iii. 15P31
iv. 19K39
the cathode if you charge a lead storage battery for 1.85 h with a constant current of 13.4 A?
How many grams of lanthanum chloride LaCl3 must be added to 1 kg of water to lower the freezing point of water by 1.1 degrees C?
what is the half life for this reaction B) how long will it take for the concentration of SO2Cl2 to decrease to 25 percent of its initial concentration C) if the inital concentration of SO2Cl2 is 1.00 M
write the structure for all iupac name for alkane with formula c6h14 that aha only primary and secondary carbon atom
Compare the volume of 1.0 g of bromine, Br2, as a solid, liquid, and gas. The density of solid bromine just below the melting point of -7°C is 3.2 g/mL, of liquid bromine at 25°C is 3.1 g/mL.
The atomic mass of boron is 10.81 g/mol. The two naturally occuring isotopes are B-10 with a mass of 10.0129 amu and B-11 with a mass of 11.0093 amu. Determine the percent of naturally occuring B-10.
Potassium reacts with oxygen to make potassium oxide, K2O. What is the maximum mass (g) of K2O(s) that could be prepared from 8.18 g of K(s) and 2.72 g of O2(g)?
determine the empirical formula of a substance (Vanillin) that contains 63.15% carbon, 5.30% Hydrogen, and 31.55% oxygen.
derive Raoul's law using the chemical potentials of the constituents that make up the mixture of the solution.
A 13.386 g aliquot of this solution is then titrated with 0.1052 M HCl. It required 30.21 mL of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste.
Find the pH of a solution that has a weak acid concentration of 1.72 M and a weak base concentration
Draw the major organic product from the reaction of 2-(carboxymethyl)benzoic acid with acetic
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