The reaction between fluorine and chlorine dioxide, F2(g) + ClO2(g) → 2FClO2(g) Proceeds according to the following rate Law: r=k⋅PF2⋅PClO2 where k= 0.0489 bar-1 s-1. In an isolation experiment, the initial partial pressures are: PF2(t=0) = 0.04687 bar and   PClO2(t=0) = 3.606 bar.   Note: Ukeff   means units of keff . You need to use a string with no spaces. For example enter gm3   as g*m^{-3} or g/m^3 . (a) Calculate the effective rate constant keff=  Ukeff=  (b) Compute the pressure of fluorine in bar after 55.8 s. PF2(t=55.8s)=  bar (c) How long will it take for the pressure of fluorine to drop to 0.01318 bar?   t =    s

The reaction A− + H+ → P has a rate constant given by the empirical expression kr = Ae−(5925 K)/T with A = 6.92 × 1012 dm3 mol−1 s−1. Evaluate the enthalpy and entropy of activation at 25 °C.

A certain reaction has an activation energy of 63.0 kJ mol−1kJ mol−1 and a frequency factor of A1�1 = 5.20×1012 L mol−1 s−1L mol−1 s−1 . What is the rate constant, k�, of this reaction at 29.0 ∘C∘C ? Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash.

Write down the kinetic equation for a simple reaction in a homogeneous medium 2A + B = 2C. Indicate the general and in relati on to all reactants reaction orders

Manfred Eigen, a German physical chemist working dur- ing the 1970s and 1980s, earned a Nobel Prize for devel- oping the "temperature-jump" method for studying kinetics of very rapid reactions in solution, such as proton transfer. Eigen and his co-workers found that the specific rate of proton transfer from a water molecule to an ammonia molecule in a dilute aqueous solution is k = 2 x 10° s-'. The equilibrium constant Kµ, for the reaction of ammonia with water is 1.8 x 10-8, What, if anything, can be deduced from this information about the rate of transfer of a proton from NH; to a hydroxide ion? Write equations for any reactions you mention, making it clear to which reaction(s) any quoted constant(s) apply.

A rate constant is found to fit the expression kr = Ae−(4972 K)/T with A = 4.98 × 1013 dm3 mol−1 s−1 near 25 °C. Calculate Δ‡G for the reaction at 25 °C; assume κ = 1.

he equilibrium NH3(aq) + H2O(l) ↔NH4+(aq) + OH−(aq) at 25 °C is subjected to a temperature jump which slightly increases the concentration of NH4+(aq) and OH−(aq). The measured relaxation time is 7.61 ns. The equilibrium constant for the system is 1.78 × 10−5 at 25 °C, and the equilibrium concentration of NH3(aq) is 0.15 mol dm−3. (a) Calculate the rate constant for the forward step. kf,eff = _____________. Just value in 3 sig. fig., normal or exponential format,  e.g. type in 1.16E6 meaning 1.16 x 106, must use capital E here. Choose a unit in the next question, must be in one of those. (b) choose a unit for the forward rate constant.     no unit     s-1     L/mol/s     L2/mol2/s

(a) Explain the meaning of the sentence:“The velocity laws of reactions are empirical” (b) It can be determined that the velocity law of a generic reaction A +B→Pév = k[A]x[B]y. Plot on a graph the variation of [A] and [P] with time, and explain why v= d[P]/dt = -d[A]/dt. (c) Explain the meaning of the terms k, x and y, in the velocity law, presented in item b: (d) Explain what it means in practice for a velocity law to be of zero order. Plot ,A as a function of t, for the zero-order reaction A→Products. (e) Explain what elementary reactions are and how they can be classified.

If the volume of a container for the reaction A+2B=C is suddenly reduced to ½ its original volume with the moles of A, B and C maintained constant, the rate will increase by a factor ofA. 2B. 4C. 8D. 16