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Problem- If Magnesium is burned under pure nitrogen, a black powder, Mg3N2 is produced. Why then is the product gray when Mg(s) is burned in air?
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What is the pH of the solution resulting from the addition of 25.0 mL of .01M NaOH solution to 40.0 mL of .01M acetic acid
Determine the equilibrium total pressure in a closed reaction flask if 0.040 mol of NO and 0.020 mol of O2 were placed in the evacuated reaction flask and heated to 100°C, resulting in a 75%-yield of NO2.
a buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 ml of 0.30 m ammonia kb 1.8 times 10-5. to this
On the basis of the solubility rules, write a balanced molecular equation for the precipitation reactions that take place when the following aqueous solutions are mixed. If no precipitation reaction is likely for the reactants given
Sketch a qualitative MO diagram for [Ni(NH3)6]2+ and identify the portion of the diagram considered by crystal-field theory. Imagine the ammonia ligands were all exchanged with a pi-donor ligand
The concentrations of each were then determined as follows: [Fe^3+]= 6.8 x 10 ^-4 M, [SCN ^-]= 3.3 x 10 ^-4 M, [FeSCN ^2+]= 3.0 X 10 ^-5 M. Determine the equilibrium constant for this reaction.
Chemistry is a natural science that deals
A 0.0100 molal aqueous solution of a weak acid freezes at -0.0219 oC. Calculate the percent ionization of the weak acid, HA.
Assuming you have avaiable to you a 50.0 g sample of glass (c=0.0837 J/g C) and a 50.0 g sample of iron (c=0.0452 J/g C). Both samples start at room temperature, 24.3C. If 500. joules of heat were added to each of these samples,
Considering the combustion of propane, how many grams of O2 are needed to completely burn 32.1g of C3H8
The specific heat of iron is 0.451 J/g·°C. If 12.04 kJ of heat energy are applied to 180.0 g of iron at an initial temperature of 22.0°C, what is the final temperature of the iron
calculate the amount of heat required to vaporize 8.48g of water at its boiling point
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