Using the results of the Arrhenius analysis (Ea = 93.1kJ/mol and A= 4.36 × 1011M-s), predict the rate constant at 299 K. Express the rate constant in liters per mole-second to three significant figures. ? L/(mol - s)

Consider this reaction: NH,OH (аq) — NH, (ад)+ н,о (ад) At a certain temperature it obeys this rate law. rate = (0.619 s)[NH,OH] S Suppose a vessel contains NH,OH at a concentration of 0.340M. Calculate the concentration of NH,OH in the vessel 2.60 seconds later. You may assume no 4 other reaction is important. Round your answer to 2 significant digits. ) M x10

The rate of a reaction of Go is .457 mol/L•min. Calculate the rate for the appearance of Hu (mol/L•min)?   3Go + HuQw3 -> 3GoQw +Hu The rate of appearance of Ae is 0.777 mol/L•min. Determine the rate of disappearance of T (mol/L•min). 2 T + Ru2 + 2 Ae3Ge -> 2 TRuGe + 6 Ae

A certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. N] [+.] H, initial rate of reaction x10 0.974 M 1.96 M 7.00 x 10 M/s 0.974 M 0.604 M | MIs 1.32 M 1.44 M Mls M/s

8 H chemPad H XX LE # Supporting Materials Periodic Table Additional Materials W 17 - Su2... → Help Greek Constants and W The reaction of fluorine and chlorine dioxide, shown below, is first order with respect to fluorine and first order with respect to chlorine dioxide. Write the rate law for this reaction. (Rate expressions take the general form: rate = k. [A]a. [B]b.) F₂(g) + 2 CIO₂ (g) → 2 FCIO₂(g) Factors G b * webassign.net 8 Supplemental Data L a ▸ G

Consider the initial-rate data at a certain temperature in the table for the reaction described by 2NO₂(g) +Q₂(g) →N₂0₂g+%₂8 Determine the value and units of the rate constant, k. k = [NO2] (M) 0.650 1.10 1.76 Units: [03] (M) 0.800 0.800 1.40 Initial rate (M/s) 3.25 x 104 5.50 X 104 15.40 X 10

The synthesis of ammonia obeys the following reaction: N2(g) + 3H2(g) → 2 NH3(g) N2(g) concentration measurements were taken at different times and plotted. 1) What is the average reaction rate of NH3(g) between 0 and 3 hours? (Attention, the graph is in "hour" and we want a speed in "mole/L s") 2) What is the instantaneous rate of reaction of NH3(g) at the 1st hour? 3) What is the general speed between 0 and 3 hours?

Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.0317 M¹-s¯¹) [₂0₂] S Suppose a vessel contains N₂O5 at a concentration of 0.440 M. Calculate the concentration of N₂O5 in the vessel 480. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ? X S

- 1 At a certain temperature the rate of this reaction is second order in H,CO, with a rate constant of 0.00683 M - 1 S. : Н,СО, (аq) — н,0 (ад)+со,(аq) Suppose a vessel contains H,CO, at a concentration of 1.01 M. Calculate the concentration of H,CO, in the vessel 580. seconds later. You may assume no 3. other reaction is important. Round your answer to 2 significant digits. | M x10 ?

What is the half life of the following reaction, given the following set of conditions (Hint: observe the units for the rate constant to determine the order of the reaction!):  2 HI (g) → H2 (g) + I2 (g)   Initial concentration of HI = 1.00 M k = 1.2 x 10-3 M-1 s-1   Select one: a. 420 s b. 240 s c. 580 s d. 830 s