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A certain monomer used in the production of polymers has one nitrogen atom and the mass composition 67.90% C, 5.70% H, and 26.40% N. Sketch the probable geometric structure of this molecule, labeling all the expected bond lengths and bond angles.
How many milliliters of a 120 mL solution of 1.51 M BaCl2 must be used to make 16 mL of a solution that has a concentration of 0.3 M Cl-?
The equilibrium lies far to the right. The reaction will proceed very slowly. The reaction contains significant amounts of products and reactants at equilibrium. The equilibrium lies far to the left.
A solution of methanol, CH3OH, cotains 55.0 grams of methanol in 100. mL of water solution. What is the molarity of methanol in the solution?
The highest possible oxidation state for halogens is +7 and the lowest possible is -1. Which of the following could not disproportionate?
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.400 M. N2(g)+O2(g) 2NO(g) If more NO is added, bringing its concentration to 0.700 M, what will the final concentration of NO be after equilibrium is r..
Calculate the number of moles of ions present in 15.1 g of a solution that is 6.30% MgSO4 by mass. What formula do you use for this problem?
A low-melting solid A was isolated, which combustion analysis showed had composition C9H10O. The substance gave a precipitate when treated with 2,4-dinitrophenylhydrazine solution.
The equilibrium constant kp for the following reaction is found to be 4.31 *10^-4 at 375 degrees C. N2(g)+3H2(g) 2NH3(g) Calculate the partial pressures of all species when equilibrium is reached.
a mixture of gases containing .20 mol of SO2 and .2 mol of O2 in a 2.0L flask reacts to form SO3. If the temperature is 25C, what is the pressure in the flask after reaction is complete?
How much heat is associated with the dissociation of a weak acid, NaHSO4 in water? HSO4^-+H20 >>> H3O^+ + SO4^2-? (not sure if this is a seperate part?) Is this dissociation exothermic or endothermic
An unknown compound has a forula of CxHyOz. You burn 0.1523 g of the compound and isolate 0.3718 g of CO2, and 0.1522 g of H2O. What is the empirical formula of the compound?
The mass percent of sulfur in the product is Blank 1 % (2 dec places). The mass percent of oxygen in the product is Blank 2 % (2 dec places).
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