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Problem- The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 . 10-3 s-1. If the initial concentration of N2O5 is 2.88 M, what is the concentration of N2O5 after 12.5 minutes?
I just need a general explanation of it please- Thanks
Calculate the energy change for the reaction K(g) + I(g) → K+(g) + I- (g) given the following ionization energy (IE) and electron affinity (EA) values. IE K = 419 kJ/mol, IE I = 1010 kJ/mol; EA K = 48 kJ/mol. EA I= 295 kJ/mol
On the basis of the general solubility rules given in the table, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. Indicate which rules apply.
The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 x 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K. Determine the activation energy for this reaction.
A mixture is 10 mole % ethyl alcohol, 75 mole % ethyl acetate and 15 mole % acetic acid. calculate the mass fractions of each compound. what is the average molecular weight of the mixture
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Define below is a carbocation intermediate in an electrophilic addition reaction of HCl with two different alkenes.
how many grams of 1,4-butanediamine and adipoyl dichloride are required to synthesis 5g of Nylom 4-6 (MW of repeat unit 198.26 g/mol)? show calculations
If iron is oxidized to Fe2+ by a copper(II) sulfate solution, and 0.519 grams of iron and 21.0 mL of 0.590M copper(II) sulfate react to form as much product as possible, how many millimoles (mmol) of the non-limiting reactant will remain unuse..
The Born-Haber process is used to determine the enthalpy of formation of common salts as it is the hardest process to measure. For KBr the enthalpy of formation follows this equation
Write a balanced equation with appropriate net ions for when solutions of potassium chromate and barium nitrate are added together.
Utilizing the periodic table arrange the atoms in each of the subsequent sets in order of increasing electronegativity.
An aqueous solution of trichloroacetic acid, that is 2.00 percent by weight trichloroacetic acid, has a density of 1.0083 g/mL. A student determines that the freezing point of this solution is -0.382 oC.
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