Consider some first-order reaction: 3 X (g)→ Y (g) + Z (g). At 534 K 22% of X changes to products in 17.3 min. (a) What is the rate constant for this reaction? (b) What is the half-life of X?
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Consider some first-order reaction: 3 X (g)→ Y (g) + Z (g). At 534 K 22%...
Consider some first-order X (g)→ Y (g) + Z (g) + U (g). The rate constant for this reaction is 2.7 x 10-4 s-1 at 750oC. Initially only X is present at a pressure of 0.520 atm. What is the pressure of the X at a constant volume after 17 minutes? EXTRA CREDIT: (+ 5 points) Calculate the total pressure of the system described in the previous question at a constant volume after 17 minutes? Hint: Both gaseous reactants and...
Consider the reaction X Y +Z Which of the following is a possible rate law? a) Rate = k[X] b) Rate = K[Y] c) Rate = k[Y][Z] Rate = k[X][Y] Rate = k[Z] e) Rate 3. What are the units for the rate constant for an overall third order reaction? a) L/mol:s b) LP/mol.s mol/L'S e) L2 For which order reaction is the half-life of the reaction inversely proportional to k, the rate constant? a) zero order b) first order...
For some second-order reaction: 2 X (g)→ 2 Y (g) + Z (g). The following data were obtained at 95°C: [A]o = 7.38 x 10-3 M [A]t = 2.67 x 10-3 M t = 720 s Calculate the rate constant for this reaction.
At 25°C, some second-order reaction 2 X (g)→ Y (g) + Z (g) has a half-life of 4.62 hours when the initial concentration of X is 3.47 M. How much X will be left after 5.6 hours?
The rate constant, k, for a first-order reaction is equal to 3.4 x 10-3 3-1. What is the half-life for the reaction?
3. (20 pts) a. Consider the following reaction: PC15(g) z PC13(g) + Cl2(g) Using the following data find the AH°, 45°, and AG° at 534 K. Kºp 0.245 1.99 4.96 9.35 T(K) 485 534 556 574 b. For the reaction above state whether the equilibrium shifts to the left or the right (or neither) when the following changes are made in an equilibrium mixture at 25 °C. 1. Tis decreased at constant P 2. Vis decreased at constant T Some...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k k and not on the reactant concentration. It is expressed as t1/2=0.693k t 1 / 2 = 0.693 k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t1/2=1k[A]0. A certain first-order reaction (A→products A → p r o d u c t s ) has a rate constant of 9.30×10−3...
3(12) The first-order reaction, 2N2O(g) + 2N2(g) + O2(g), has a rate constant of 0.76 s at 1000K. (a) Calculate the half-life of this reaction at 1000K. (b) How long will it take for the concentration of N20 to fall to 25% of its initial value at 1000K (c) How long will it take for reaction to be 90% complete? (d) If the half-life of the same reaction is 29 min at 800K, what is the rate constant at 800K?...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant concentration. It is expressed as t 1/2 = 0.693 k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t 1/2 = 1 k[A ] 0 Part A A certain first-order reaction ( A→products ) has a rate constant of 9.90×10−3 s −1 at 45 ∘...
2. Answer the following questions by connecting the half-life of each first-order reaction to the rate constant. a. The rate constant of a first-order reaction is 2.43 × 10–2 min–1. What is the half-life of the reaction? (2 points) b. A first-order reaction has a rate constant of 0.547 min-1. How long will it take a reactant concentration 0.14 M to decrease to 0.07 M? (2 points) c. The half-life of a first-order reaction is 5.47 min. What is the...