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The evaporation of a 120-nm film of n-pentane from a single crystal of aluminum oxide is zero order with a rate constant of \(1.92*10^{13} \frac{molecules?}{cm^{2}*s}\) at 120K.
a. If the initial surface coverage is 8.9*10^16 molecules/cm^2, how long will it take for one-half of the film to evaporate?
b. What fraction of the film is left after 10 s? Assume the same initial coverage as in part a.
calculate the mass in kilograms of 3.99 liters of acetic acid. the density of this substance is 1.05g/mL ?
What is the pH of a solution containing 0.001 M NaHCO3 and 0.002 M NH3? You may assume that both the carbonic acid system
Compute the Ka for the acid if the pH of the resulting solution = 6.36. and determine the pH of the resulting buffer
Identify the qual 1 cation that is confrimed present in a reference solution by the formation of a precipitate? by the color of a soluble complex ion?
A modern chealting agent used for this purpose is succimer (C4H6O4S2). Suppose you are trying to determine the appropriate dose for succimer treatment of lead poisoning.
Use the de Broglie relationship to determine the wavelengths of the following objects: an lithium atom moving at 2.5*10^5m/sUsing Heisenberg's uncertainty principle,
One of those bands consists of radio waves with a wavelength near 20.m . Calculate the frequency of these radio waves. Be sure your answer has the correct number of significant digits.
A jogger runs at an average speed of 5.9 mi/h. a. How fast is she running in m/s? b. How many kilometers does she run in 98 min?
What is the expected freezing point of an aqueous solution of 2.62 kg of nitric acid, HNO3 , in a solution with a total mass of 5.91 kg? Assume that the nitric acid is completely ionized.
What is the volume in mL of 0.585 M HCl(aq) needed to reach halfway to the equivalence (stoichiometric) point in the titration
When 0.100g of graphite is burned completely in a bomb calorimeter(heat capacity =3.344kJ/?C), containing 3000 g of water, a temperature rise of 0.21?C is observed.
What is a significant obstacle when using osmometry to determine molar masses for compounds with very high molar masses? A. The osmotic pressures may be too high to measure.
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