The decomposition of dinitrogen pentoxide obeys the tart-law expression rate = 0

Question

The decomposition of dinitrogen pentoxide obeys the tart-law expression rate = 0.080 min^-1[N_2O_3]. If the initial concentration of N_2O_3 is 0.30 M, what is the concentration after 2.6 minutes? N_2O_3 rightarrow N_2O_3 + O_2 a. 0.38 M b. 0.13 M c. 0.028 M d. 0.24 M e. 0.32 M Which one of the following would force the forward reaction to completion? CaCO_3(s) 2H_3O^+(aq) Ca^2+(aq) + 3H_2O(l) + CO_2(g) a. Adding CO_2 to the reaction mixture. b. Adding more Ca^2+ to the mixture. c. Removing some H_3O^+ from the reaction mixture, by neutralizing it with base. d. Removing CO_2 as it is formed. e. None of the preceding would have any cf?cct on the amount of CaCO_3 consumed. When balancing oxidation-reduction reactions, all of the foUowina apply except. a. The electrons must always cancel in the balanced reaction. b. There must be mass balance. c. The balanced reaction will always have a zero charge on both sides of the equation. d. Half-reactions are balanced finst, and then added. e. There must be charge balance. Given the following data for theNH_4^+ + NO_2^- rightarrow N_2 + 2H_2O reaction The rate law for the reaction is a. rate = k[NH_4^+]^2[NO_2^-] b. rate = k[NH_4^+][NO_2^-]^2 c. rate = k[NH_4^+]^2[NO_2^-]^2 d. rate = k[NH_4^+][NO_2^-] e. None of the above

Explanation / Answer

1) rate = 0.080 min-1 [N2O5]
K = 0.080 min-1 , the reaction is first order reaction
   ln[A] = ln [Ao] - Kt
   ln[A] = ln [0.30] - 0.080*2.6
   ln [A] = -1.4119728
   [A] = e-1.4119728 = 0.24366
   option d is the answer
2) According to the Le Chatlier's principle
   Removing H3O+ , adding CO2 or adding Ca+2 to the mixture will result in backward shift
   Removing CO2 as it is formed is the right answer as it only helps the reaction to move forward.
option d is the answer
3) option b, is the answer you do not perform mass balance for redox reactions
4) option d is the answer

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