For the reaction, 2COF_2(g) implies CO_2(g) + CF_4(g), K_e = 2.00 at a particula

Question

For the reaction, 2COF_2(g) implies CO_2(g) + CF_4(g), K_e = 2.00 at a particular temperature. A reaction mixture at this temperature initially contains all three gases in equal concentrations. Which is true of this reaction mixture? Q K: the reaction proceeds toward the reactants The reaction A rightarrow products obeys second order kinetics. What is the concentration of A remaining after 2.00 minutes if the reaction has a rate constant of 0.0482 M^-1 s^-1 and the initial concentration of A is 0.379 M. 0.0655 M 0.119 M 0.366 M 8.42 M Determine the reaction order with respect to [A] for the reaction A + B + C rightarrow products [A]/M [B]/M [C]/M initial rate/M.min^-2 0.100 0.100 0.100 3.00 times 10^3 0.0.100 0.100 0.200 6.00 times 10^3 0.200 0.200 0.200 2.40 times 10^4 0.100 0.200 0.200 2.40 times 10^4 0 1 1.5 2 According to the collision theory for chemical reactions, why do most reaction rates increase as temperature is increased? At higher temperatures The concentration of reactants increase. the activation energy of the reaction decreases. more molecules collide with the necessary energy. more molecules have the proper orientation when they collide. A chemical reaction is performed at 200 K and at 400 K. The reaction has activation energy of 50.0 kJ-mol^-1. At 400 K the rate of reaction is the same as the rate at 200 K. approximately double the rate at 200 K. approximately 200 times the rate at 200 K. over 3 million times the rate at 200 K. A drug is metabolized in a first order reaction with a half-life of 4.12 days. If a patient ingests 100.0 mg of this drug, what mass remains after 30.0 days? 0.391mg 0.441 mg 0.643 mg 0.672 mg The reaction HNC(g) implies HCN(g) is first order in [HNC]. Which plot is correct for this reaction? Consider this reaction mechanism Step 1 NO_2(g) + Cl_2(g) implies_k_1 ClNO_2(g) + Cl(G) (slow) Step 2 NO_2(g) + Cl(g) + Cl(g) implies_k_2 ClNO_2(g) (fast) Overall Reaction 2NO_2(g) + Cl_2(g) implies 2ClNO_2 (g) The overall reaction is order with respect to NO_2 and order with respect to Cl_2.2nd, 2nd 2nd, 1st 1st, 2nd 1st, 2nd 1st, 1st Which energy diagram best illustrates a reaction that is thermodynamically favored but kinetically slow?

Explanation / Answer

32. calculating the reaction quotient (Q) we get that that Q=1, which implies that the reaction will proceed in the forward direction as Ke=2. Therefore, option (A).

33. 1/[A] = 1/[Ao] + kt, putting the values given we get the answer as (B).

34. As seen form the 3rd and 4th row values we see that when the concentration of A is changed (reduced to half) we get no change in the rate of reaction, which implies that with respect to A the order of reaction is 0. option (A).

35. (C). at higher temperature the reactants have higher energy so higher entropy so higher probability of collision.

36. using Arhenius equatio for rate of reaction = Ae-Ea/RT and putting the values of temperature for both the cases we get option (D).

37. Using first order rate law => kt = ln(Ao/A) and using the value of k calulated from the relation => t1/2 = .693/k, we get the mass of drug after 30 days as 0.6434 mg. option (C).

38. (B), using first order rate equatio as in question 37.

39. option (B), looking at the stoichiometric coefficients in the overall reaction.

40. option (B), because the energy of the product is less than energy of reactants so thermodynamically favoured while the activation energy is quiet high so kinetically slow.

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