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Half-life of first order processA reactant undergoes a dissociation reaction A r arrow 2B which follows first order kinetics. The initial concentration of reactant A is .4000 M and after 75.00 hr the concentration of A decreases to 0.0816 M. Determine the half-life of the first order process.
There must be a simple equation for this, but my textbook must assume we would already know it. I can't find it anywhere
the heat of combustion of butane is -2878kj/mol assume a typical cigarette litter hold about 1.75 grams of butane how much energy would be released
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Calculating concentration at equilibrium, The equilibrium constant Kc for the reaction is 54.3 at 430 deg C
What is the molarity of a solution prepared by dissolving 13.1 g of glucose (of MW 180 amu) in 217 mL of solution?
If one mole of ATP yields 7 kcal of energy, how much energy would be available from the anaerobic catabolism of 270 g of glucose (C6H12O6)? Show your work.
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