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Freons are compounds that contain carbon, chlorine, and fluorine in various proportions. They are used as foaming agents, propellants, and refrigeration fluids. Freons are controversial because of the damage they do to the ozone layer in the stratosphere. A 5.87 g sample of a particular freon in a 3.45 L bulb at 25.00°C has a pressure of 262.00 torr. What is the molar mass of this compound? Enter units.
Use a drawing program to draw a beaker.
A mixture of 1 atm chlorine gas and 1 atm oxygen gas and no product undergoes this reaction. Cl2 + 2 O2 ---> 2 ClO2 What equation would be used to solve for the equilibrium concentrations
What is the kinetic energy of the emitted electrons when cesium is exposed to UV rays of frequency \rm 1.5\times 10^{15}~Hz
Consider two samples of liquid: one mole of water H2O and one mole of ethanol C2H5OH. The density of water is 1.0 g/mL, and the density of ethanol is 0.785 g/mL. Answer each of the following questions by selecting the correct choice.
determine the maximum number of coordination sites that the ligand can occupy on a single metal ion.
Draw a detailed mechanism for the formation of 1,4-di-t-butyl-2,5-dimethoxybezene from t-butyl alcohol.
Determine how long will it take for a sample of N2O5 to decay to sixty percent of its initial value?
Zinc has two isotopes. Zn-64 has an atomic mass of 63.9292amu and Zn-72 has an atomic mass of 71.9278amu. Its average atomic mass is 65.38amu. Calculate the abundance, in percent, of Zn-64.
What is the pressure of a container that has 7 atm pressure coming from O2, 2 atm of pressure coming from N2, 3 atm of pressure coming from CO2?
Aluminum readily displaces hydrogen in sulfuric acid according the following balanced reaction: 2Al(s) + 3H2SO4(aq) = Al2(SO4)3(aq) + 3H2(g). How many moles of Al and how many moles
Compute pH and [OH-] for each of the following solutions. (a) 8.1×10-2M Na2CO3, (b) 0.15M NaCN
Predict what will happen and check your predictions. Change the styling so that instead of the color changing the link becomes bold when you hover over it. (You need to use the font-weight property.) Why does the white background extend to the end..
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