2. Consider the second order reaction 2NOB → 2NO+ Br2 The rate constant is 0.80 M-1...
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s) at 10°C. Starting with a concentration of 0.86 M, calculate the concentration of NOBr after 59 s.
The rate constant for the second-order reaction: 2NOBr(g) → 2NO(g) + Br2(g) is 0.80/(M · s) at 10°C. Starting with a concentration of 0.86 M, calculate the concentration of NOBr after 89 s. M
Enter your answer in the provided box. The rate constant for the second-order reaction: 2NOBr(g) + 2NO(g) + Br2(g) is 0.80/( M s) at 10°С. Starting with a concentration of 0.86 M, calculate the concentration of NOBO after 67 s. L M
The rate constant for the second-order reaction: 2N02(g)-→ 2NO(g) + O2(g) is 0.54/M s at 300°C 2 M to 0.28 Mn (a) How long (in seconds) would it take for the concentration of NO2 to decrease from 0.6 (b) Calculate the half-lives at these two concentrations.
The reaction 2NOB → 2NO+ Br2 exhibits the rate law Rate = k[NOBr] = A[NOBr) A: where k = 1.0 x 10-5 M-1.5 at 25° C. This reaction is run where the initial concentration of NOBT ([NOBr]) is 1.00 x 10- M. Calculate the [NO] (M) after 3.6 hours have passed. Report your answer to two significant figures. Answer:
The rate constant for the second order reaction 2 NO2 ⟶ N2O4 is 2.79 M-1.min-1 at 48oC. If the initial concentration of NO2 is 1.05 M, what is the half-life?
1. A certain first order reaction has a rate constant of 0.036 min-1. How much of the reactant will remain if the reaction is run for 2.5 hours and the initial concentration of the reactant is 0.31 M? 2. A certain first order reaction has a rate constant of 0.036 min-1. How much of the reactant will remain if the reaction is run for 2.5 hours and the initial concentration of the reactant is 0.31 M? 3. The rate constant...
The reaction 2A → B is second order with a rate constant of 51.0/M · min at 24 ° C. (a) Starting with [A]0 = 9.30 ×10−3M, how long will it take for [A]t = 2.80 ×10−3M? min (b) Calculate the half-life of the reaction. min
9. The reaction 2A → B is second order with a rate constant of 51.0/M·min at 24°C. (a) Starting with [A]0 = 9.50 × 10−3M, how long will it take for [A]t = 3.10 × 10−3M? ______ min (b) Calculate the half-life of the reaction. _______ min 10. The thermal decomposition of phosphine (PH3) into phosphorus and molecular hydrogen is a first-order reaction: 4PH3(g) → P4(g) + 6H2(g) The half-life of the reaction is 35.0 s at 680°C. a) Calculate...
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...