Consider the following reaction and initial rate data: 2 NO(g)  +  O2(g)  -->  2 NO2(g) Trial Initial NO conc., M Initial O2 conc., M Initial Rate, M/s 1 0.0126 0.0125 0.0141 2 0.0252 0.0250 0.113 3 0.0252 0.0125 0.0564 The rate order with respect to NO is                             [ Select ]                          ["0", "1", "2", "3"]            . The rate order with respect to O2 is                             [ Select ]                          ["0", "1", "2", "3"]            .

A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. initial rate of reaction x10 0.537 M 0.350 M 21.0 M/s 0.169 M 0.350 M || M/s 0.261 M 0.721 M M/s

[A] vs Time In[A] vs Time O 1/[A] vs Time Least Squares Plot The reaction A → C was performed and the concentration vs. time data below collected. time, s [A], mol/L 0.7983 0.1898 0.1077 0.07517 0.05774 0.04687 0.03944 0.03405 0.02995 [A] 0 reaction order = Check Submit Answer 1 Time, s 2 3 Try Another Version Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = K[A]* rate constant (without units) = Next> (1 of 1) Show Approach 2 item att 5 6 Hide Hint 7 8 A least squares line gives the best straight- line fit through any set of points but to get the right answer you need to figure out which plot gives the straight line.

don't reject no honour code in this question