The reaction: 2 N2O5(g) 4 NO2(g) + O2(g) rate = K [N205]? %3D If the half-life for this reaction is 43.9 minutes, and the original concentration is 0.35 M what is the rate constant, (k)? O 2.32 x 10-3 M.s O 1.32x 10-3 M.s O 1.085 x 10-3 M1s O 1.085 x 10-3 M.s

Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A] where k= 3.00×10-3 s-1 at a particular temperature. If the initial [A] = 0.500 M, what will be the concentration of A after 2.00 minutes? 0.497 M 0.349 M 0.424 M 0.499 M

Payalben

For the reaction 203(g) --> 30₂(g), the following mechanism was proposed: step 1: 03(g) --> O₂(g) + O(g) step 2: O(g) + 03(g) --> 2 O₂(g) If step 1 is the slow step, the reaction would be [Select] for 03 and [Select] for 02. If step 2 is the slow step, the reaction would be [Select] for O3 and [Select] for O₂.

Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A]2 where k= 1.45 ×10-2 M-1s-1 at a particular temperature. If the initial [A] = 0.300 M, what will be the concentration of A remaining after 3.00 minutes?  0.168 M 0.0221 M 0.296 M 0.287 M

The rate of a certain reaction is given by the following rate law: rate =k N, O, Use this information to answer the questions below. olo What is the reaction order in N,? |x10 18 Ar What is the reaction order in 03? What is overall reaction order? At a certain concentration of N, and 03, the initial rate of reaction is 0.780 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 5.0 x 103M/s when [N2] = 1.1 M and [03] = 1.1 M. Calculate the value of - 3 -1 k = |M •S the rate constant. Round your answer to 2 significant digits.

A reaction has the following rate law: Rate = k [A] [B]2 If the rate = R at some concentrations of A and B what is the expected rate if the concentrations of both A and B were doubled?       2R     4R     8R     16R

just need  standard error  for K

In a study to determine the rate of the following reaction: 2NO(g) +0,(g) 2NO, (g) the concentration of NO was 0.0650 Mat t= 5.0 s and 0.0225 Mat t= 650.0 s. What is the average rate of the reaction during this time period? M/s

You have a reaction: A + B --> C The reaction is first order with respect to A and 2nd order with respect to B. If 1.3 mol of A is mixed with 2.3 mol of B to make a 1.000 L solution and the rate of the reaction is 1.6 M/s, what is the rate constant (k)?