Question

6. The initial rates listed in the table below were determined for the reaction CO(g) + NO2(g) + CO2(g) + NO(g) at varied concentration of the reactants, CO and NO2. Determine the rate law of this reaction. Experiment Initial [CO] (mol/L) Initial [NO] (mol/L) Initial rate (mol/Ls) 5.0x10+ 3.5x10 3.4x10-8 5.0x10+ 7.0x10- 6.8x10-8 1.5x10 3.5x10 1.02x10-7 7. The half-life of the reaction C&H:(8) ► 2CH.g) at constant temperature is independent of the reactant concentration. What is the order of this reaction in C&H ? 8) Which of the following statements about a "order reaction a Products is false? A. The rate law of such reaction is: Rate-k[A]. B. The integrated rate law of such reaction is: In[A]:--kt+In[A]o. C. When the initial concentration of A is doubled, the rate is doubled as well. D. The plot of In[A] vs. time is linear. E. The half-life is determined by the formula: t12 - 1/([A]ok). 9. What are the units of the rate constant, k, for the following rate law: Rate =k[A][B]'? 10. Initial concentration of reactant A in a 2nd-order reaction A - Products is 0.880 M. In 30 min, the concentration of A decreases to 40.0% of its initial value. Determine the rate constant of this reaction. 11. Rate constants for the reaction N2O(g) 2 NO2(g) are 2.5x10 s at-5.0 °C and 3.5x10 s at 25 °C. Calculate the activation energy E. (in kJ/mol) for this reaction. 12. For a particular 1"-order reaction, the rate constant at 30.0 °C is 0.271 s ! The activation energy of this reaction is 125 kJ/mol. Find the rate constant of this reaction at 60.0 °C.

can you do the 6-12 number 8 is multiple choice

Answer 1

I (6) Consider the Rate Law is Rate :k [co]*[Nog] 3.4*100% from exp 1 & exp (2) = k (5.0810-4 2 68x10-8 *15-0X105)& (20x10-5) B 2 = (12) 3 [B=1 from exp I & exp 3 3.4X10-8. *(56710-(3.5X10ss) 1.08 x 107 ☆ (1.5x10°3)– ( 315x76-55 Rate = k [60] [102] for order : 1 , half life is undependent of 7 reactant concentration typ = 0.693 ) (8) first order Reaction Rat= K[A]2 order. untegrated Rate laws = Im[Ale=- kt ten [40] This equation utself reveal that en[A] vi t is simple knear equation plot.

» As explained in above question, tip2= D.693. In this formula no concentraron of reactant came. Hence, Opton E is correct answer no contention optional (9) Ratta k [A] [B] Unit of Rate = Ms1 o concentration : M Un MS = R(M) (M) ² Mst=R (M)3 MStze => R= Modes ka (covec) -?time)] M3
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