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Millikan's oil drop experiment gave charges -3.204 E -19 C, -4.806 E-19 C, -8.010 E -19 C, -1.442 E -18 C what is the smallest charge? (HINT: it's not the smallest number written here).
Which of the bonding forces from the list above would need to be overcome to convert CCl4 from a liquid to a gas? (Enter the letters in order of all that apply, e.g. AB, ABD, ACDE, etc.)
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.
Pu-239 (nuclear mass of 239.0006 amu) decays by alpha emission to U-235 (nuclear mass of 234.9934). Calculate how much energy is given off by the decay of 2.00 mg of Pu-239.
Determine the amount of kJ that is needed to heat 45 grams of water that is at 25.0 °C and until it all boils away?
What is the volume percent of a solution prepared by dissolving 43 g of NaOH in enough water to make a final volume of 120 mL? Show your work.
At 320 K and 16 atm pressure, the molar volume of ammonia, NH3, is about 10% less than the molar volume of an ideal gas. The best explanation for actual volume being this much smaller than ideal volume is that
Carbon monoxide gas burns in oxygen to form carbon dioxide gas. Write a balanced equation for the reaction and determine the volume of oxygen needed to react completely with 174 mL of CO at 40.0°C
When 1.150 grams of an unknown nonelectrolyte dissolves in 10.0 grams of water, the solution freezes at -2.16°C. What is the molecular weight of the unknown compound? Kf for water = 1.86°C/m.
An aqueous solution is 8.50% ammonium chloride, NH4Cl, by mass. The density of the solution is 1.024 g/mL. Explain what are the molality, mole fraction, and molarity of NH4Cl in the solution
Why cultured animal cells can survive in the absence of linoleic acid
What mass of NH4Cl should the student dissolve in the solution to turn it into a buffer with pH =8.77
Problem- Determine the concentrations of each zinc-containing species in a solution saturated with solid Zn(OH)2 and having a fixed OH- concentration of 3.7 x 10-7 M. The equilibrium constants for the equilibria that occur in the solution follow:
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