The reaction of ammonium ion with nitrite ion in aqueous solution NH, + NO. →N₂ + 2H₂O is first order in NHA and first order in NO₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate= In an experiment to determine the rate law, the rate of the reaction was determined to be 3.72 x 105 M-s¹, when [NH,"]= 0.564 M and [NO₂] = 0.164 M. From this experiment, the rate constant is M¹.s

The gas phase reaction of hydrogen with iodine H₂+ 12 → 2HI is first order in H₂ and first order in I2. Complete the rate law for this reaction in the box below. Use the form [A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate In an experiment to determine the rate law, the rate constant was determined to be 2.39 x 10-18 M's. Using this value for the rate constant, the rate of the reaction when [H2]=0.0636 M and [12]=0.0154 M would be M/s. Submit Answer Retry Entire Group more group attempts remaining

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The decomposition of nitramide, O₂NNH,, in water has the chemical equation and rate law [O₂NNH₂] [H+] O₂NNH, (aq)- -N₂O(g) + H₂O(1) A proposed mechanism for this reaction is 1.0,NNH, (aq) = O,NNH(aq) + H+ (aq) (fast equilibrium) rate = k 2.0, NNH (aq) N₂O(g) + OH- (aq) (slow) 3. H(aq) + OH-(aq) H₂O(l) (fast) What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism? k₂ Answer Bank k_ k3 k

The reaction of nitrogen dioxide with fluorine 2NO2+F2-->2NO2F is first order in NO2 and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A]^m[B]^n, where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n .

What is the rate constant for the reaction?

Q2

The reaction of UO,* with hydrogen ion in aqueous solution 2 UO,* + 4 H* → U** + UO2²* +2 H2O is second order in UO,* and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A]™[B]"... , where 'l' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate =

In a particular reaction, BrO3- + 5 Br- + H3O+ → 3 Br2 + 9 H2O , the following table below is completed with the initial concentrations of each reactant and the initial rate for each trial. 1.) Write the rate expression for this reaction. (HINT: rate = -Δ[rcts]/Δt = +Δ[pdcts]/Δt ... )  2.) Write the rate law for this reaction. (HINT: rate = k [rcts]x ... ) 3.) What is the overall order for this reaction? 4.) What is the rate constant (k) for this reaction? Extra Credit: Calculate the rate of this reaction when [BrO3-] = 0.50 M, [Br-] = 0.25 M, and [H3O+] = 0.35 M.

The reduction of nitric oxide with hydrogen 2NO+2H₂ → N₂ + 2H₂O is second order in NO and first order in H₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 7.99 x 10-³ M-s¹, when [NO] = S = 0.192 M and [H₂] = 0.129 M. From this experiment, the rate M².s¹. constant is