A reactant, A, decomposes according to a first order rate law. It takes 3.5 hours for 25% of A to decay. (10) How many grams of A will be left over after 75 minutes, if there are 10.0 g initially?
A reactant, A, decomposes according to a first order rate law. It takes 3.5 hours for...
The rate law for a general reaction involving reactant A is given by the equation rate = k[A]?, where rate is the rate of the reaction, k is the rate constant, [A] is the concentration of reactant A, and the exponent 2 is the order of reaction for reactant A. What is the rate constant, k, if the reaction rate at 450.°C is 1.23x10-1 mol/L.s when the concentration of A is 0.220 mol/L? 1/Mos When heated to 75°C, 1 mole...
At a particular temperature, N2O5 decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N2O5 is 1.0 × 1016 molecules/cm3, what will be the concentration in molecules/cm3 after 11.5 s? A. 7.0 × 1014 B. 3.4 × 101 C. 1.0 × 1016 D. 2.0 × 1014 E.
first order reaction First-Order Reactions (35) Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g) — N2(g) + C2H6(g) The following data are obtained in an experiment: Time (h) [(CH3)2N2] 1.00 0.905 2.00 0.741 3.00 0.607 4.00 0.497 (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time in hours) that it takes decrease the concentration to 0.100 M. (d) Calculate...
A first order rate law has a rate constant of 0.0011 s-1. If the initial concentration is 4 M. How much is left after 9 minutes?
The rate constant for a first order reaction is 0.20 M-1s-1. The time it takes for 0.50 M of reactant to halve is________ s 1.2 2.5 3.5 10
Gaseous azomethane, CH3N=NCH3 , decomposes in a first-order reaction when heated: CH3N=NCH3(g) ---->N2 (g) + C2H6 (g) The rate constant for this reaction at 600 K is 0.0216 . a. If the initial quantity of azomethane in the flask is 4.64 g, how much remains after 0.0510 hour? b. how many grams of N2?
1a. Hydrogen iodide decomposes when heated, forming H2 (g) and I2 (g). The rate law for this reaction is -delta[HI]/delta t = k[HI]^2. At 443 °C, k=30.L/molxmin. If the initial HI (g) concentration is 5.5x10^-2 mol/L, what concentration of HI (g) will remain after 10. minutes? Concentration = ____ mol/L 1b. The decomposition of SO2Cl2 SO2Cl2 (g) ----> SO2 (g) + Cl2 (g) is first-order in SO2Cl2, and the reaction has a half-life of 245 minutes at 600 K. If...
1. For a first order decay of [A], if 525 mg remains of an initial sample of 1.3079 g after 361 min, what is the half life (in minutes)? 2. The decay of antimony-131 is first order with a half life is 23.03 minutes. How much of 1.4228 g sample would remain after 1.368 hours? 3. The decay of antimony-131 is first order with a half life is 23.03 minutes. How long (in minutes) would it take for a 0.8893...
16. Order: Aminophylline 0.75 g IV in 500 mL DSW to run for 4 hours Rate: ml/h 17. Order: 1.5 L NS to infuse over 16 hours Rate: 18. Order: 750 mL LR to infuse over 6 hours Rate:1mL/h 19. Ms. Costales is treated for diabetic ketoacidosis. The label on the insulin drip states 2500 units/500 mL DSNS. If the IV infuses at 10 mL/h, how many units is the client receiving per hour? a. 5 units/h b. 25 units/h...
A certain reactant disappears by a first order reaction that has a rate constant K= 3.5x10^-3 s-1. If the initial concentration of the reactant is 0.500 M , how long will it take for the concentration to drop to 0.200 M ? 4. A certain reactant disappears by a first-order reaction that has a rate constant k=3.5 x 10 s. If the initial concentration of the reactant is 0.500 M, how long will it take for the concentration to drop...