The data of the initial rate experiment of the following reaction are given below. The rate law expression of the reaction is Rate = k[S208 J*[ r}Y. Determine the rate constant k with 3 significant figures (key-in only your value; no units are needed). Note that your k value should be reported based on second (the time units here). Do not covert second to other time units. S208° (aq) + 3 I" (aq) → 2 so4²" (aq) + 13` (aq) (S20g Jo (M) [rJo (M) initial rate (M/sec) Trial 1 0.800 0.140 0.0288 Trial 2 2.400 0.140 0.2592 Trial 3 0.800 0.280 0.0288 Note that Trial 1 and Trial 3 have the same initial rate.

5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T

A value of k is found from the rate equation Rate = k[A]m[B]n. If m=1 and n=4 and -1 the unit for the initial rate is M/h. The unit of k is found to be MX h-¹ (M to the power of x h to the power of minus 1). What is the value of x?

For the reaction: NO (g) + O3 (g)  ---> NO2 (g) + O2 (g) the value of A= 8.7 x 1012 s-1 and Ea = 63 kJ/mol. What is the value of the rate constant k for the reaction at 75oC? Enter your answer in units of s-1 to 2 significant figures. Enter your answer in the format:  a.b x10^m, where a.b and m are the appropriate numbers based on your calculation.

Determine the average rate of change of B from t O s to Time (s) Concentration of A (M) t = 282 s. 0.740 141 0.465 A - → 2B 282 0.190 rateB M/s

Consider a reaction: A+ B → C and the rate law expression: Rate = k [A]M[B]^ %3D In the rate law expression above, what do 'm' and 'n' determine? order of reaction concentration of A and B they have no significance I have no idea