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If the rate constant of a first order reaction is 4.87X10-5 s-1 at 15 degrees C compute the rate constant at 80 degrees C if the activation energy is 250 Kj/mole (R=8.314J/K)
Describe how to got it and each part of the formula
Borazine B3 N3H6 is isoelectonic with benzene. Explain qualitatively the bonding in this molecule in resonance as well as molecular orbital theory.
A 2.18 g vitamin C tablet was melt in water. It took 28.45mL of 0.124 mol/L sodium hydroxide to neutralize the ascorbic acid in the tablet. Compute the percent (m/m) of ascorbic acid in the tablet.
Briefly explain which indicator, bromocresol purple (pKa = 6.3; from yellow to purple) or thymolphthalein (pKa= 10.0; from colourless to blue), would be better for use in this titration
0.10 grams 1, 3, 5-trichlorobenzene, 0.10 grams 2- chloronaphthalene as well as 0.10 grams biphenyl, dissolved individually in three 100ml samples of benzene.
One mole of an ideal monoatomic gas initially at 300 K is expanded from an initial pressure of 10 atm to a final pressure of 1 atm. The molar heat capacity for constant volume for the gas is 32VCR=. Calculate dU, dH, q, w, and the final temperatur..
Determine the pH of the acid solution before the titration begins and the pH at the equivalence point when 50.0 mL of the NaOH has been added. The Ka of HF is 7.2*10^-4
Calculate the detection limit (90% and 95% confidence interval) for a single measurement. Use the equation D.L = (ks)/m
Determine theoretical yield, limiting agent and excess reagent - How much excess reagent remains after the reaction goes to completion
Calculate the amount of heat transferred when 46.0 g of CH3OH is decomposed by this reaction at constant pressure.
Copper has two isotopes: Cu-63 (abundance = 69.2%, mass = 62.930 amu) and Cu-65 (abundance = 30.8%, mass = 64.928 amu). Calculate the (average) atomic mass of copper.
A sample of unknown hydrate of FeCl3 weighs 8.693g. After heating the sample to constant mass, the remaining anhydrous salt weighs 5.216g. What is the experimental formula for the hydrate
Consider the following gas-phase reaction: NO2(g) + N2O(g) 3 NO(g) Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions
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