How to calculate the reaction orders (using experimental data) and write the rate law for a...

How to calculate the reaction orders (using experimental data) and write the rate law for a reaction

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Using the data in the table, calculate the rate constant of this reaction.

Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+DA+B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.290 0.240 0.0197 2 0.290 0.528 0.0953 3 0.522 0.240 0.0355 ?= Units=

Using the data listed below, determine the rate law and the rate constant for this reaction...

Using the data listed below, determine the rate law and the rate constant for this reaction at 60°C with respect to hypochlorite decomposition. t (min) [ClO-] (M) 0 0.950 60 0.941 120 0.932 240 0.915 360 0.898 480 0.882 720 0.851 1080 0.809 1440 0.771 1800 0.736 2160 0.705 2520 0.676 2880 0.649 3600 0.601 4320 0.560 5040 0.524 5760 0.493 6480 0.465 7200 0.440

Given the following data and using Hess’ Law, Calculate change in Enthalpy for the reaction Overall...

Given the following data and using Hess’ Law, Calculate change in Enthalpy for the reaction Overall reaction : CH4(g) + 2 O2 (g) ------> CO2(g) + 2H2O(l) 2H2O(l) ------> 2H2O(g) ∆H = 88 kJ CH4(g) + 2 O2 (g) ------> CO2(g) + 2H2O(g) ------> 2O(g) ∆H = -802 kJ

Given the following data and using Hess’ Law, Calculate change in Enthalpy for the reaction Overall...

Given the following data and using Hess’ Law, Calculate change in Enthalpy for the reaction Overall reaction : NO(g) + O (g) ------? NO2(g) 2O3(g) ------? 3O2(g) ?H = - 427 kJ O2(g) ------? 2O(g) ?H = 495 kJ NO(g) + O3 (g) ------? NO2 (g) + O2 (g) ?H = - 199 kJ

Find the rate law expression and the rate law constant for the reaction whose data is...

Find the rate law expression and the rate law constant for the reaction whose data is in the table below. Trial [X] [Y] Rate 1 2.0 2.0 2.5 x 10—6 2 2.0 6.0 2.25 x 10—5 3 4.0 2.0 2.0 x 10—5 b. Calculate the rate of the reaction described in part a) when [X] = 0.25 mol/L and [Y] = 6.0 mol/L.

For this important smog reaction the experimental rate law is r=kexp [NO]^2[O2]. a.) Show that the...

For this important smog reaction the experimental rate law is r=kexp [NO]^2[O2]. a.) Show that the following mechanism is consistent with the rate law and identify keep proposed mechanism. NO+NO<--> N2O2 fast k1/k-1 N2O2+O--> 2 NO2 slow k2 b.) What is the function of N2O2 and how do you know? c.)What is the difference between a catalyst and an intermediate ? d.) Activation energies are: 82(r1), 205(r-1, and 82(r2) kJ/mol. If the Arrhenius pre-exponential factors all approximately the same what...

Calculate the enthalpy of reaction for the following reaction using Hess's Law and the equations provided...

Calculate the enthalpy of reaction for the following reaction using Hess's Law and the equations provided below. Target Reaction: Sr(s)+C(graphite)+1 1/2 O2(g) -----> SrCO3(s) H(degrees)=? C(Graphite)+ O2(g)-----> CO2(g) H(degrees)= -349kJ Sr(s)+ 1/2 O2(G)-------> SrO(s) H(degrees)= -592kJ SrO(s)+CO2(g)-------> SrCo3(s) H(degrees)= -234kJ

1. Based on your experimental determined rate law for the reaction of crystal violet and hydroxide ion, how would doubling the concentration of crystal violet affect the reaction rate?

Trial 1 Time Trans A=2-log %T Ln(A) 1/A 1:57 19.0 0.721 -0.327 1.39 2:52 22.0 0.658 -0.419 1.52 3:51 24.5 0.611 -0.493 1.64 4:54 27.3 0.564 -0.573 1.77 5:53 29.7 0.527 -0.641 1.90 6:54 33.6 0.474 -0.747 2.11 7:55 36.2 0.441 -0.819 2.27 8:54 40.0 0.398 -0.921 2.51 9:52 40.5 0.393 -0.934 2.54 10:53 45.3 0.344 -1.07 2.91 11:58 47.7 0.321 -1.14 3.12 13:02 52.2 0.280 -1.27 3.57 14:02 55.3 0.257 -1.36 3.89 14:59 56.0 0.252 -1.38 3.97 15:59 59.4...

Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [A]...

Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [A] (M) [B] (M) Rate (M/s) 1 0.280 0.240 0.0160 2 0.280 0.576 0.0922 3 0.504 0.240 0.0288 k= Units

Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [?]...

Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.350 0.300 0.0161 2 0.350 0.750 0.101 3 0.490 0.300 0.0225 k= _________? Mention the unit as well

Subjects