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245.0 nm ultraviolet light strikes a metal plate and ejects electrons having kinetic energy E = 1.79 eV. Calculate the binding energy of an electron at the metal surface.
calculate the minimum number of grams of C3H8(g) that must be combusted to provide the energy necessary to convert 2.93 kg of H2O from its solid form at -13.0°C to its liquid form at 75.0°C.
What mass of sucrose should be combined with 483 of water to make a solution with an osmotic pressure of 8.50 at 320 ? (Assume the density of the solution to be equal to the density of the solvent.)
When a sample of H2S(g) (9.811 mol) is placed in 180.0 L reaction vessel at 724.0 K and allowed to come to equilibrium the mixture contains 0.01627 mol/L of S2(g). What is the equilibrium concentration (mol/L) of H2S(g)? 2H2S(g) = S2(g)+2H2(g)
A student mixes 175.0 grams of water at 62.31oC in a coffee-cup calorimeter with 175.0 grams of water at 25.84oC. The final temperature of the mixture is 41.71oC.
The density of a sample of an unknown solid is 16.9 g/cm3. Convert this density to to units of lb/ft3.
Using the appropriate equation from your lecture notes, how much of a 5 gram sample will be extracted from 20mL of water using 15mL of an organic solvent and the partitian coefficient is K = 0.50.(nearest hundredth)
Draw every stereoisomer for 1-bromo-2-chloro-1,2-difluorocyclopentane. Use wedge-and-dash bonds for the substituent groups, and be sure that they are drawn on the outside of the ring, adjacent to each other
What's more significant an affect on atomic size, an increase in nuclear charge or increase in occupied energy levels within a group
how many grams of sodium lactate should be added to 1.00 of 0.150 lactic acid to form a buffer solution with 4.00?
Calculate the pH at each of the following points in the titration of 50.0 mL of a 0.95 M B(aq) with 0.95 M HCl(aq).
Given the equilibrium constants below: (1/2) N2(g) + (1/2) O2(g) NO(g) Kc= 4.8*10^(-10) 2 NO2(g) 2 NO(g) + O2(g) Kc= 1.1*10^(-5) What is the equilibrium constant for: 2 NO2(g) N2(g) + 2 O2(g) Kc=?
A buffer solution contains 0.23 mol of carbonic acid (H2CO3) and 0.55 mol of sodium hydrogen carbonate (NaHCO3) in 2.10 L. The Ka of carbonic acid (H2CO3) is Ka = 4.3e-07. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer af..
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