The reaction A + B → P is found to be first order in both A and B. The reaction was carried out in a solution that was initially 0.080 mol dm−3 in A and 0.060 mol dm−3 in B. After 1.0 h the concentration of B had fallen to 0.030 mol dm−3. (i) Calculate the rate constant. (ii) What are the half-lives of the reactants?

1a) Calculate the rate constant (with appropriate units) for a first order reaction which is 32.0% complete in 380 s. 1b) What is the value of the half-life of the reaction? 1c) How long will it take for the reaction to go to 76.0% completion?

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

The acid-catalyzed hydrolysis of sucrose occurs by the fol-lowing overall reaction whose kinetic data are given below:C₁₂H₂₂O₁₁(s)  H₂O(l) →C₆H₁₂O₆(aq)  C₆H₁₂O₆(aq) (a) Determine the rate constant and the half-life of the reaction.(b) How long does it take to hydrolyze 75% of the sucrose?(c) Other studies have shown that this reaction is actually sec-ond order overall but appears to follow first-order kinetics.(Such a reaction is called a pseudo–first-order reaction.) Sug-gest a reason for this apparent first-order behavior.

In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is (1.37x10^0)/s. Fe3+(aq) + SCN-(aq)  → Fe(SCN)2+(aq). What is the half-life, in seconds, of the reaction? Express your answer to three significant figures.

You determine through experimentation that the reaction A⟶P is first order with respect to A. If the rate constant of the reaction is determined to be 5.58 x 108 s−1, what is the half-life when [A]= 0.352 M at 25 ∘C. τ1/2 in seconds

The decomposition of nitramide in aqueous solution at 25 °c NH2NO2(aq)N½O(g) + H20(1) is first order in NH2NO2. During one experiment it was found that when the initial concentration of NH2NO2 was 0.402 M, the concentration of NH2NO2 dropped to 7.40x10-2 M after 25187 s had passed. Based on this experiment, the rate constant for the reaction is s-1.

Under certain conditions, the reaction 3 A+ 4B 5C is observed to proceed at a rate of 0.0275 M s ¹. What is the corresponding rate of change in product C?

The recombination reaction 2 HO₂(g) → H₂O2(g) + O₂(g) has a second-order rate constant of 1.8E9 M1 s1. Calculate the half-life of the reaction if the initial concentration of HO₂(g) is 1.7E-11 M. Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is: 1/c = 1/co+2kt Include at least 3 significant figures in your answer. Show Transcribed Text

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.