Question

Can you explain with all necessary steps and equations? thank you

4. Use the method of initial rates (the simple method, not the more robust approach) to determine the rate law and rate constant for the reaction NH + NO3 - N2 + 2 H2O (acid solution) Given the following data: [HNO2]/M [NH *] / M. Rate x 108/mol Li's! 0.0092 0.098 34.9 0.0092 0.049 16.6 0.0488 0.196 335 0.0249 0.196 156

Answer 1

Thanks!

Solution: NH4 + 0 N9 + 2 ,o (acid & Pion) Rate dow: - According to Rate dow date of reaction 18 a faction of intial concentration of the reactants. Rate = k [NG] [NO] Where K Rade constant [N Hqf] - Concentration of NHqt iong [NO ] → Concentration of Ngions from Given Data [no] = 0.0092M, CNHHJ = 0.098 m and Retre x 108-34.9 from aan mol[lseil 34.9 = K (0.098) (0.0092) 108 K = 38708.9618x 108 I'mod sect K = 3.87 X 70422' mai'sec! from and Dada 16056 = K (0.0092) (0-049) => k = 36823.42X108 K = 3168 X1012 et meil sec 1 from me Date 335 = K (0-196) (0.0488) >> K = 35024.25x168 K = 3.50x102 I'mot sec) 1 from oth Data 156 = *(0.196) (0.0249) = K = 31964-59X108 K = 3.19 x 1012 I'mot 'sect 102 108