The table gives initial rates for the reaction 2A + B rightarrow C + D starting

Question

The table gives initial rates for the reaction 2A + B rightarrow C + D starting with different concentrations of A and B. What is the rate law for the reaction? (A) Rate = k[A][B] (B) Rate = k[A]^2[B] (C) Rate = k[A][B]^2 (D) Rate = k[A]^2[B]^2 What is the rate of decomposition of chromate ions (CrO_4^2-) if the rate of formation of dichromate ions (Cr_2O_7^2-) is 0.30 M middot s^-1? 2CrO_4^2- (aq) + 2H^+ (aq) rightarrow Cr_2O_7^2- (aq) + H_2O(l) (A) 1.20 M middot s^-1 (B) 0.60 M middot s^-1 (C) 0.30 M middot s^-1 (D) 0.15 M middot s^-1 What do X and Y represent in this diagram? (A) X + Y is the enthalpy of reaction. (B) X is the activation energy and Y is the enthalpy of reaction. (C) X is the energy of the transition state and Y is the activation energy (D) X is the enthalpy of reaction and Y is the energy of the transition state. The reaction of ozone with NO_2, 2NO_2 + O_3 rightarrow N_2O_5 + O_2, contributes to the is depletion of ozone in the atmosphere. Which rate law is consistent with this proposed mechanism for the reaction? NO_2 + O_3 rightarrow NO_3 + O_2(slow) NO_3 + NO_2 rightarrow N_2O_5 (fast) (A) Rate = k[NO_3][NO_2] (B) Rate = k[NO_3][O_2] [C] Rate = k[NO_2][O_3] (D) Rate = k[NO_2]^2[O_3]

Explanation / Answer

Q40

if

Cr2O7-2 is forming at 0.3 M/s

then, ratio is 1:2 so

0.6 M/s for CrO4-2 in order to satisfy stoichiometric ratio

choose B

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