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Balance the following equation in basic solution. indicate which reactant becomes oxidized during the reaction, which reactant becomes reduced, which is the oxidizing agent, and which is the reducing agent. IO3- +NO2- ---> I- +NO3-
If 37.3 g of CO2 is produced in the reaction of C2H2 with O2 to form CO2 and H2O, how many grams of H2O are produced in this reaction.
Determining System Equilibrium, A one-litre cylinder at 458'C is found to contain 0.36 moles of HI (g), 0.15 moles of I 2(g), and 0.18 moles of H2(g). Is this system at equilibrium?
Acid, Bases and Proton Transfer, what is the direction of proton transfer?
4.00g of H2SO4 solution was diluted with H2O and added with excess of cacl2, and The washed and dried precipitate of BaSO4 weighted 4.08g. Calculate percent H2SO4 in the original acid solution.
How much energy (in kilojoules) is required to convert 110 mL of diethyl ether at its boiling point from liquid to vapor if its density is 0.7138 ?
Write a complete stepwise mechanism for the reaction of cyclopentanone with bromine in acetic acid to give 2-bromocyclopentanone. Show all intermediate structures and all electron flow with arrows.
The DHfus of ethanol (C2H5OH) is 4.60 kJ/mol. How many kilojoules of heat are required to melt 24.5 g of ethanol at its freezing point.
At constant external pressure (1.2atm), the temperature of 3.25 mol of ideal gas increased from 250K to 305K. Calculate the internal energy change ΔE.
A certain solid metallic element has a density 7.87 g/cm3 and a molar mass of 55.85 g/mol. It crystallizes with a cubic unit cell, with an edge length of 286.7 pm. calculate the number of atoms per unit cell.
A 248 mL gas sample has a mass of 0.436 g at a pressure of 753 mm Hg and a temperature of 27 degrees celcius.what is the molar mass of the gas
The specific heat of Ti is .523 J/gcelcius. What is the final temperature of 62g of Ti intially at 41celcius after 8.5kj of heat is added?
Suppose that the solvent ethanol could serve to replace the methanol in this process, but at the expense of double the concentrations of the solvent in the atmosphere.
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