At 45°C the rate constant is 6.2 x 10 s. The reaction is first order. a What is the rate law for the reaction? Rate = k[N2O5] [NO,)*[O2] Rate = k[N2 Os] %3D Rate k[NO,] [O2l Rate = k[N2O5] b Calculate the rate of the reaction when [N2O5] is 0.40 M. Rate = |M/s

The rate of a certain reaction is given by the following rate law: rate = k[NO] [0,] Use this information to answer the questions below. What is the reaction order in NO? What is the reaction order in 02? What is overall reaction order? At a certain concentration of NO and O2, the initial rate of reaction is 0.270 M / s. What would the initial rate of the M reaction be if the concentration of NO were halved? Round S your answer to 3 significant digits. the reaction is measure — 0.60 М and [O-] The rate to be 62.0 M / s when - 1 - 2 k = ||M [NO] 1.2 M. Calculate the value of the •S rate constant. Round your answer to 2 significant digits.

Dinitrogen pentoxide, N205, decomposes by a first order reaction with an activation energy of 110 kJ/mol. At 65 °C, the rate constant is k = 5.2 x 10-3 s-1. What is the initial rate of reaction when 8.01 g of N,O5 is confined in a 0.75 liter container and heated to 65 °C? A. 3.98 x 10-4 M/s B. 5.14 x 10-4 M/s C. 0.56 x 10-5 M/s D. 2.31 x 10-2 M/s

Consider the reaction and its rate law. 4A + 3B What is the order with respect to A? order: products What is the order with respect to B? order: What is the overall reaction order? overall order: rate = k[A]²[B]²

It was found that for the reaction 2 A + B → 3 C the rate law is Rate = k[A][B] · %3D At the initial concentrations [A]o = 0.100 M and [B]o = 0.200 M the initial rate is 0.0500 M/s. %3D What would be the initial rate if the initial concentrations were [A]o = 0.500 M and [B]o = 0.0750 M? 0.0352 M/s 0.0937 M/s O 0.0711 M/s 0.00533 M/s O 0.469 M/s

Question is attached.

The exponents in a rate law describe the effects of the reactant concentrations on the reaction rate and define the reaction order. Consider a reaction for which the rate law is: rate = k[A]m[B]n If m is 1, the reaction is first order with respect to A. If the exponent is 2, the reaction is second order with respect to A. If n is 1, the reaction is first order in B. If m or n is zero, the reaction is zero order in A or B. If m = 1 and n = 1, the overall order of the reaction is second. (m + n = 1 + 1 = 2). 1. What is the difference between a reaction rate and a reaction's rate constant? 2. What does it mean if a reaction is zero order with respect to a reactant?  3. Doubling the concentration of a reactant increases the rate of a reaction four times. What is the order of the reaction with respect to that reactant? 4. Doubling the concentration of a reactant increases the rate of a reaction four times. Tripling the concentration of a different reactant increases the rate of a reaction…

Would this be zero order ?

The rate of a certain reaction is given by the following rate law: =k[N₂]²[H₂]² Use this information to answer the questions below. rate What is the reaction order in N₂? What is the reaction order in H₂? What is overall reaction order? At a certain concentration of N₂ and H₂, the initial rate of reaction is 71.0 M/s. What would the initial rate of the reaction be if the concentration of N₂ were halved? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 0.930 M/s when [N₂] = 0.79 M and [H₂] = 0.88 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. M 04/1 S -3 1 k = M ²³.5²¹ S

Consider the rate law: Rate = k[NO][O,] Which of the following statements is FALSE regarding this rate law? O The value of k will increase with temperature. O The reaction is 2nd order overall. O The reaction is 1st order with respect to O2 The reaction is 2nd order with respect to NO.