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Light having a wavelength of 2.50x10^-7 m falls upon the surface of a piece of chromium in an evacuated glass tube. If the work function of chromium is 7.26x10^-19 J, determine (a) the maximum kinetic energy of the emitted photoelectrons and (b) the speed of photoelectrons having this maximum kinetic energy.
A buffer solution of pH of 9.25 contains P mol of a weak base and Q mol of a salt of its conjugate acid. When 120 cm3 of a 0.0140 mol.dm-3 solution of hydrochloric acid was added to this buffer solution
How is hydrogen bond different from an ionic or covanlent bond?
A chemist wants to prepare a solution with a freezing point of 22.0°C and has 100.00 g of glycerol on hand. What mass of water should the chemist mix with the glycerol?
What is an alternative analytical procedure for determining the quanity of water in a non-aqueous sample?
What is the molarity of ZnCl2 that forms when 30.0 grams of zinc completely reacts with CuCl according to the following reaction? Assume a final volume of 275.
the density of milk is 1.04 g/ml, how many milligrams of milk are in 0.50 qt of milk? (1L=1.057 qt, 1000g=1Kg, 1000ml=1L, 1000mg=1g)
What happens to the time at which the mid point of the breakthrough curve exists the column if the particle size is halved but the adsorption isotherm and column size stay the same?
Why can the nature of the metal salt precursor be changed during the epoxide addition method so easily without altering
When a container is filled with 3.00 mol of H2 , 2.00 mol of O2 , and 1.00 mol of N2 , the pressure in the container is 465 kPa. The partial pressure of O2 is ?
How many grams of Cuso4 are needed to prepare a .150 molal solution in 300 grams of water?
A 1.00 g sample of enriched water, a mixture of H2O and D2O, reacted completely with Cl2 to give a mixture of HCl and DCl. The HCl and DCl were then dissolved in pure H2O to make a 1.00 L solution
Use the graph of solubility of O2 in water vs. temperature to calculate the value of Henry's law constant KH
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