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The decomposition reaction X → products was studied as a function of time. Data are given in the table below.
What is the value of the rate constant? |
The decomposition reaction X → products was studied as a function of time. Data are given...
The decomposition reaction, X → products, has rate constant k = 0.00741 mol−1 L s−1. How long will it take for the decomposition to be 80% complete, if the initial concentration of X is 1.35 mol L−1 ?
The reaction X + Y → products was studied using the method of initial rates. The initial rate of consumption of X was measured in three different experiments. Data are provided below. Expt [X]0 (in mol L−1) [Y]0 (in mol L−1) Initial Rate (in mol L−1 min−1) 1 0.500 0.500 0.4338 2 1.25 0.500 1.084 3 0.500 0.750 0.9759 What is the order of the reaction with respect to X? (Enter an integer.) What is the order of the reaction...
The decomposition of NOBr is studied manometrically because the number of moles of gas changes; it cannot be studied colorimetrically because both NOBr and Br2are reddish-brown. 2NOBr(g) ? 2NO(g) + Br2(g) Use the data below to make the following determinations: (a) the average rate of decomposition of NOBr over the entire experiment. (b) the average rate of decomposition of NOBr between 2.00 and 4.00 seconds. Time (s) [NOBr] (mol/L) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00...
a) Given these data for the reaction , write the rate-law expression. (Use k for the rate constant.) Rate = _______ The specific rate constant = ___________ Expt. Initial [A] (M) Initial [B] (M) Initial Rate of Formation of C () 1 0.15 0.40 4x10^-5 2 0.15 0.80 1.6x10^-4 3 0.30 1.6 1.3x10^-3 b) The rate of the elementary reaction C2H2 + H2->C2H4 has been studied as a function of temperature between 300 and 2500 K. The following data were...
The rate of decomposition of azomethane is studied by monitoring the partial pressure of the reactant as a function of time. The data obtained at 300°C are listed on the right. Determine the rate constant of the reaction at this temperature. time: 0, 100, 150,200,250,300 P (mmHg): 284,220,193, 170,150,132
3. The thermal decomposition of A, 2A + products is a second-order reaction. Given that the initial concentration of A is = 2.45 x 10-3 M and the intial rate of reaction is 2.05x10-6 M s-1, calculate the rate constant. Also calculate the rate of reaction after 90% of A has reacted.
please write neat and explain steps, thank you
4. The decomposition of glitterstim (an illegal drug) was studied, and the following data were obtained at a particular temperature: Table 1. Decomposition of glitterstim by exposure to light. Time (s) 0 12 56 2 (glitterstim] (mol/L) .56 x 102 2.47 x 102 2.16 x 10-2 1.31 x 102 5.19 x 10 2.73 x 10 Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate (glitterstim)...
The gas phase decomposition of N2O5(g) àNO3(g) + NO2(g) is studied at a certain temperature, giving the following data: Time (s) [N2O5] (M) 0.0 1.000 50.0 0.677 100.0 0.458 150.0 0.310 200.0 0.210 Is the overall order of reaction zeroth, first or second order? What is the rate constant (include units)? Calculate half-life (in s) for this reaction given the initial concentration in the table. What is the concentration of N2O5 (in M) at 250. s?
1. The kinetics of the following reaction have been studied: N2
+ 3 H2 → 2 NH3 The rate of of appearance of NH3 was measured as
∆[NH3]/∆t = 9.00 x 10-2 mol L-1 s-1
(a) What is the rate of the reaction in mol L-1 s-1?
(b) What is ∆[N2]/∆t in mol L-1 s-1?
(c) What is ∆[H2]/∆t in mol L-1 s-1?
2. The initial rate of the reaction of species A and B A + 2 B →...
The reaction A(aq) +B(aq) - Products(aq) was studied, and the following data were obtained: [Alo (mol/L) [Blo (mol/L) Initial rate (mol/L.) 0.32 0.48 0.16 0.32 6.17x10-1 2.06x10-1 7.72x10-2 6.17x10-1 0.080 0.24 0.64 0.24 The order of the reaction in A is