2- (a) At some point in the reaction 2A + B G+ 3H, [A]=0.3629 M. At a time 8.25 min later [A] = 0.3187 M. What is the average rate of formation of H during this time interval, %3D expressed in M/s? (b) The first order decomposition reaction of N2O5 is given as follows; N2O5 (in CCL) → N»O4 (in CCL4) + ½ O2(g) Find the rate constant (k) corresponding to a 2.00 h half-life at 25°C. Calculate the half-life of the given decomposition reaction at 32°C, if the activation energy is 106 kJ/mol? (R:8.314 J/mol.K)

A student proposed the following mechanism for the gas phase reaction of fluorine with chlorine dioxide. step 1 fast: 2 CiO,=Cl,04 step 2 slow: Cl,0, + F2→2 FCIO, (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"|B]".. , where 'l' is understood (so don't write it if it's a '1') for m, n etc. Rate =

The reaction 2 NO(9) + 02 (9) → 2 NO2(9) was studied, and the following data were obtained where A[02] Rate = At NOo [02]o Initial Rate (molecules/cm³) (molecules/cm) (molecules/cm° · s) 1.00 x 1018 1.00 x 1018 2.00 × 1016 3.00 x 1018 1.00 x 1018 1.80 x 1017 2.50 × 1018 2.50 × 1018 3.13 x 1017 What would be the initial rate for an experiment where [NO], = 2.66 × 1018 molecules/cm° and [O2]o 1.48 x 1018 molecules/cm°? Rate = |molecules/cm³ . •S

The gas phase decomposition of dinitrogen pentoxide at 335 K N,O5(g)- →2 NO,(g) + ½ O2(g) is first order in N,Og with a rate constant of 4.70×10-3 s. If the initial concentration of N,0g is 0.175 M, the concentration of N,Og will be 2.15x102 M after have passed.

The gas phase reaction of iodine with silane takes place according to a second-order reaction: I2(g) +SİH4(g)–→HI(g) +SIH3I(g) The activation energy is Ea = 83.2 kJ mol-1. At 269°C, the reaction rate constant is 3.49 L mols. (a) Calculate the Arrhenius factor A for this reaction. L mols1 (b) Calculate the rate constant for this reaction at 235°C. L molls1

Be sure to answer all parts. The reaction between NO2 and CO to produce NO and CO2 is thought to occur in two steps: Step 1: NO2 + NO2     NO + NO3 Step 2: NO3 + CO     NO2 + CO2 The experimental rate law is rate = k[NO2]2. (a) Write the equation for the overall reaction. Do not include phase abbreviations.      (b) Identify the intermediate(s).     NO3    NO2    NO    CO2    CO (c) Identify the rate-determining step.     Step 1    Step 2    Neither step

The initial rate of the reaction is determined for different initial conditions, with the results listed in the table. (a) What is the overall reaction order? (b) What is the value of the rate constant, k

At a certain temperature the rate of this reaction is second order in NH4OH with a rate constant of 0.0770M NH₂OH(aq) → NH3(aq) + H₂O (aq) Suppose a vessel contains NH4OH at a concentration of 0.500M. Calculate how long it takes for the concentration of NH4OH to decrease by 77.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. 0 : x10

Be sure to answer all parts.The reaction2A → Bis second order in A with a rate constant of 37.9 M−1 · s−1 at 25°C.(a) Starting with [A]0 = 0.00701 M, how long will it take for the concentration of A to drop to 0.00180 M?s(b) Calculate the half-life of the reaction for [A]0 = 0.00701 M.s(c) Calculate the half-life of the reaction for [A]0 = 0.00215 M.

Consider the reaction 5B1¯ (aq) + Br0, (aq) + 6H† (aq)→3B12 (aq) + 3H2O(1) The average rate of consumption of Br is 1.16×10-4 M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval? Express your answer with the appropriate units.