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One mole of H2O(g) at 1.00 atm and 100.°C occupies a volume of 30.6 L. When one mole of H2O(g) is condensed to one mole of H2O(l) at 1.00 atm and 100.°C, 40.66 kJ of heat is released. If the density of H2O(l) at this temperature and pressure is 0.996 g/cm3, calculateΔEfor the condensation of one mole of water at 1.00 atm and 100.°C.
How do fluorescent dyes, like pyranine, change their structure when the dyes intensity changes, and they change brightness?
describe the preparation of 400 mL of a solution that is 0.0500 M in I-, starting with MgI2.
The bright-red color of highway safety flares comes from strontium ions in salts such as Sr(NO3)2 and SrCO3. Burning a flare produces strontium ions in excited states,
how much thermal energy is evolved by a reaction in a calorimeter in which the temperature of the calorimeter and water
Metals and nonmetals can react with each other to form ions. Complete these statements. A potassium atom gain or loses(electrons/protons/neutrons)and to form how many ion?
Describe all the symmetry planes in the staggered conformation of ethane. Draw a figure and arrows to show any rotational symmetry axes in the staggered conformation of ethane.
The value of delta E for a system that performs 213 kJ of work on its surroundings and loses 79 kJ of heat is kJ
What is the molarity of hydrogen ion in the above sulfuric acid solution if you assume the sulfuric acid ionizes completely? the above sulfuric acid solution is 0.07 M.
The reaction described in Part A required 3.50L of calcium chloride. What is the concentration of this calcium chloride solution
Suppose you were to heat the copper in argon gas instead of atmospheric gasses. Given that argon is relatively inert, which of the following would you expect if you were to heat pure copper in the presence of argon gas?
The specific heat capacity of the solution produced was 4.20 J/g•°C, and final temperature reached was 34.91°C. How much heat was produced by the dissolution
Draw the pictures of the overlap of the atomic orbitals to make all of the molecular orbitals and for any non-bonding orbitals as well.
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