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137Cs decays by beta minus emission to an isomeric state in 137Ba which then decays by the emission of a gamma-ray. If we start with a 4 mCi of pure 137Cs, define what will be the activity of 137mBa after five minutes? The half-lives of 137Cs as well as 137mBa can be found in a chart of the nuclides.
Dihydroxybenzene and o-dihydroxybenzene can be separated by TLC using silica gel and a solvent of medium polarity. The ortho isomer has a significantly higher Rf value than the para isomer. Suggest a reason for this difference in Rf values.
Draw the structure for the major Diels-Alder product of the reaction betwen 1,3-cyclohexadiene and fumaric acid, the trans isomer of maleic acid.
cadaverine a foul smelling substance produced by the action of bacteria on meat contains 58.55 c 13.81 h and 27.40 n by
What is the balanced cell reaction for the following echem cell set-up. Pt(s) / PbO2(s) / Pb(NO3)2, HNO3 // Cr(NO3)3 / Cr(s)
Copper metal is purified by electrolysis. How much copper metal could be produced from copper(II) oxide by applying a current of 10.0 amps
8h aq 5fe2aq mno4-aq -------- mn2aq 5fe3aq 4h2olthe mn is clearly reduced and is the oxiding agent how do you
Predict the partial vapour pressure of HO above its solution in liquid germanium tetrachloride of molality 0.10 mol kg-I
Solutions of strontium hydroxide, silver nitrate, hydrogen phosphate, potassium nitrate, and copper (II) sulphate are prepared and placed in separate containers. Consider the reaction of the pairs of these compounds.
The pH at 25 °C of an aqueous solution of the sodium salt of p-cresol (NaC7H7O) is 11.60. Calculate the concentration of C7H7O- in this solution, in moles per liter. Ka for HC7H7O is equal to 6.7E-11.
Until 200 yr ago manufactured iron contained charcoal created from freshly cut wood that was added during the smelting process. As a result of this practice older samples of iron can be dated accurately utilizing the carbon-14 method.
Using standard potentials given in the appendices, calculate the standard cell potentials and the equilibrium constants for the following reactions
A typical automobile gets 30 miles per gallon of gas and drives 12,000 miles every year. Assuming that octane (C8H18, density 0.7025 g cm-3) is a principal component of gasoline
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