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In regards of the subsequent mechanism. Step 1- 2A to B+C equilibrium Step 2- B+D to E slow. Overall- 2A+D to C+E. Find out the rate law for the overall reaction where the overall rate constant is represented as k.
Explain what would you expect to be the major product of nitration of 2-methylacetanilide. Define reasoning with reference to the nitration of 4-methylacetanilide.
Bromine is a reddish-brown liquid. Calculate its den-sity (in g/mL) if 650 g of the substance occupies 188mL.
What is the pH of the solution at equivalence point. How many mL of HCl will need to be added to the methlamine, CH3NH2 solution to reach a pH of 10.64. What will the major species in solution be when 1198.75 mL of HCl has been added to the base s..
monoprotic acid. Dihydrogen pthalate (H2C8H4O4) is a diprotic acid. An analyte sample contains 0.127 M KHP and 0.0678 M (H2C8H4O4). What volume of a 0.205 M NaOH solution is required to neutralize 25.0 mL of the analyte solution.
At 25 degrees Celsius, the reaction: H3O+ + NH3 --> NH+ + OH- is first order in each reactant, and has a rate constant of 4.3x 10^10 M^-1 s^-1
What is the uncertainty of the position of the bacterium. Express your answer numerically in meters.
Compute the concentration of [HPO4]2- and [H2PO4]- at pH 5.60 in a solution containing one mol of phosphate per liter (pKas for phosphate: 2.14, 6.86, 12.4)
The decomposition of ozone in the upper atmosphere is facilitated by NO. The overall reaction and the rate law are O3 + O ---> 2O2 rate = k[O3][NO]
Explain what will be the partial pressure of di-t-butyl peroxide after 1.00 hr if its initial partial pressure was 169.0 torr? Explain what will be the total gas pressure after 1.00 hr
If pH = 6.4, calculate the molar concentration of H^+ (aq) in the solution. If pH = 6.4, calculate the molar concentration of OH^-(aq) in the solution.
Hydrogen cyanide is produced industrially by the following exothermic reaction. 2 NH3(g) + 3 O2(g) + 2 CH4(g)---> 2 HCN(g) + 6 H2O(g) Is the high temperature needed for thermodynamic or kinetic reasons
Dinitrogen pentoxide, N2O5, decomposes in the gas phase to form nitrogen dioxide, NO2, and oxygen gas, O2. The reaction is first order in dinitrogen pentoxide and has a half-life of 2.81 hours at 25 C.
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