How long will it take for the concentration of A to decrease from 1.25 M to 0.401 for the second order reaction A → Products? (k = 1.52 M'min*)
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- 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.The reaction for the decomposition of ammonia into its elements ist 2 NH (a) Na (a) +3 Ha (a) [H.)= 0.414M, If the concentrations at a certain time are: [N] 0.0105 M [NH) = 0.505M what will be the associated value of the reaction quotient (a)? (A) (B) (C) 0.00148 0.00292 0.00861 (D) (E) 0.0105 3427) For the reaction CO(g) + 3 H2(g) = H2O(g) + CH4(g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M, [H2] = 0.045, [H2O] = 0.020, 7) %3D %3D %3D and [CH4] = 0.031, in which direction will a reaction occur and why? A) it is at equilibrium because Q = 190 B) toward products because Q = 4.1 C) toward reactants because Q = 0.24 D) toward products because Q = 0.38 %3D %3D %3D %3D E) toward reactants because Q = 61 %3D
- We noted in an earlier Practice Exercise that at 25 °C thedecomposition of N2O5(g into NO2(g) and O2(g) followsfirst-order kinetics with k = 3.4 x 10-5 s-1. How long willit take for a sample originally containing 2.0 atm of N2O5 toreach a partial pressure of 380 torr?(a) 5.7 h (b) 8.2 h (c) 11 h (d) 16 h (e) 32 hWhat is the effect of catalyst on:(i) Gibbs energy (ΔG) and(ii) activation energy of a reaction?If the activation energy for a reaction is 60.6 kJ/mole, how many times faster is the reaction at 500 K than 300 K? 430 6.1 O 1.7x104 O 9.7 Thermodynamic relationships: T(K) = T(°C) + 273.15 AG = AH - TAS AG = -RT In(K) R=0.008314 kJ/(mol·K) %3D (-AH RT AS ) K = e R Kinetic relationships: Integrated rate laws: zero order: [C):= [C]o-kt first order: In[C] = In[C]o-kt second order: 1/[C]. =1/[C]o+kt E. E 1 kT.. Е, 1 + In( A) R T RT2 k = Ae RT In( k) = a. = e %3D k T,
- 8) Reaction in diluted solution proceeds as follows: A I→P Describe the steady state condition of this reaction in the two ways: a) by the formula (and explain any symbols), and b) by the narrative of the same.Provided the reaction A + 2B + C → 2D + E, and the set of data thatfollows:The rate constant for the reactionBr(g)+O3(g) --> BrO(g)+O2(g)was determined at the four temperatures shown in the table below. T (K) k [cm3/(molecule•s) 238 5.90 x 10-13 258 7.70 x 10-13 278 9.60 x 10-13 298 1.20 x 10-12 Plot the above data, and then use that data to calculate the activation energy for this reaction.
- (b) Explain what will happen to the activation energy and pre-exponential factor if the following changes were made: Addition of catalyst to the system. Increasing the temperature by two-fold. (i) (ii)(a) A reaction 2 A →P has a second-order rate law with k = 3.50 × 10−4 dm3 mol−1s−1. Calculate the time required for the concentration of A to change from 0.260 mol dm−3 to 0.011 mol dm−3 (b) For the ideal gas reaction A + B ↔ 2C + 2D, it is given that ∆Gθ500= 1250 cal mol-1. If 1.0 mol of A and 1.0 mol of B are placed in a vessel at 500 K and P is held fixed at 1200 torr, calculate the equilibrium amount of A, B, C, and D.(b) Explain what will happen to the activation energy and pre-exponential factor if the following changes were made: (1) (ii) Addition of catalyst to the system. Increasing the temperature by two-fold.
