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Trial H2 (M) N2 (M) Initial rate (M/s) 1 0.00200 0.0100 2 0.00200 0.0150 8.00 x...
1A. 2NO(g) + 2H2(g) → N2(g) + 2H2O (g) EXPERIMENT [NO]0 [H2]0 Initial rate (M/s) 1...
1A. 2NO(g) + 2H2(g) → N2(g) + 2H2O (g) EXPERIMENT [NO]0 [H2]0 Initial rate (M/s) 1 0.200 0.122 0.0313 2 0.400 0.122 0.1250 3 0.200 0.244 0.0625 Using the information above, find the order of each reactant and then find the rate constant. 1B. The decomposition of dinitrogen pentoxide happens by the following: 2N2O5 (g) → 4NO2(g) + O2(g) Calculate the average rate (M/s) of decomposition given: Time [N2O5] 10 minutes 1.238 x 10-2 20 minutes 0.926 x 10-2 If...
2 ICl + H2----->I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1...
2 ICl + H2----->I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.129 8.70×10-2 1.67×10-3 2 0.258 8.70×10-2 3.34×10-3 3 0.129 0.174 6.68×10-3 4 0.258 0.174 1.34×10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = ____________ From these data,...
The reduction of nitric oxide with hydrogen 2 NO + 2 H2—+N2 + 2 H20 is...
The reduction of nitric oxide with hydrogen 2 NO + 2 H2—+N2 + 2 H20 is second order in NO and first order in H Complete the rate law for this reaction in the box below. Use the form k[A]”[B]"..., where 'l' is understood for m. n ... (don't enter l) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.82 M-5....
The reaction A→BA→B has been experimentally determined to be second order. The initial rate is 0.0100...
The reaction A→BA→B has been experimentally determined to be second order. The initial rate is 0.0100 M/sM/s at an initial concentration of AA of 0.100 MM. Part A What is the initial rate at [A]=0.400M[A]=0.400M? What is the initial rate at ? 0.00250 M/sM/s 0.160 M/sM/s 0.0100 M/sM/s 0.0400 M/s
The decomposition of ammonia on a platinum surface at 856 °C NH31/2 N2 + 3/2 H2...
The decomposition of ammonia on a platinum surface at 856 °C NH31/2 N2 + 3/2 H2 is zero order in NH3 with a rate constant of 1.50×10-6 M s-1. If the initial concentration of NH3 is 7.92×10-3 M, the concentration of NH3 will be M after 4.29×103 seconds have passed.
1. The kinetics of the following reaction have been studied: N2 + 3 H2 → 2...
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 →...
10. Initial rate data have been determined at a certain temperature for the gaseous reaction: 2NO...
10. Initial rate data have been determined at a certain temperature for the gaseous reaction: 2NO + 2 H2 → N2 + 2 H20 [NO], [Hz]. Initial Rate (M/s) 0.10 0.20 0.0150 0.10 0.30 0.0225 0.20 0.20 0.0600 The numerical value of the rate constant is: (what are the units?) a. 380 b. 0.75 c. 7.5 d. 3.0 x 10-3
over the 11. In the reaction CLC) + 3F18) -- 2 CIF), if the average rate...
over the 11. In the reaction CLC) + 3F18) -- 2 CIF), if the average rate first 6.00 s, how much CIF, will form during this time S 2CFL the d ance of F, Fis 0250 -0.250 0.750 M b. 1.00 d. 2.00 M 1.50 M 3.00 M 12. Given the following data in the der of the reaction with respe 2 NO(g) ) - 2 NOCIS) Experiment INOT (M) 0.0300 0.0150 ICI (M) 0.0100 0.0100 0.0-400 Rate (M )...
Lab Questions 1. Use the Method of Initial Rates to determine the complete rate law for...
Lab Questions 1. Use the Method of Initial Rates to determine the complete rate law for the reaction: 2 NOg)+ H2(g)-> N24g) +2 H20g) Trial [H2] 0.0100 0.0200 0.0300 0.0100 0.0100 NO Initial Rate, M/s 3.82 x 10- 7.63 x 103 1.14 x 102 1.53 x 102 3.43 x 102 20.0100 2 00100 30.0100 0.0200 0.0300 4
A certain reaction is second order in N2 and first order in H2. Use this information...
A certain reaction is second order in N2 and first order in H2. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N2] [H2] initial rate of reaction 0.229 M 2.33 M 57.0 M/s 0.111 M 2.33 M __________M/s 0.0482 M 11.1 M ___________M/s
The reduction of nitric oxide with hydrogen 2 NO + 2 H2—+N2 + 2 H20 is second order in NO and first order in H Complete the rate law for this reaction in the box below. Use the form k[A]”[B]"..., where 'l' is understood for m. n ... (don't enter l) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.82 M-5....
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 →...
10. Initial rate data have been determined at a certain temperature for the gaseous reaction: 2NO + 2 H2 → N2 + 2 H20 [NO], [Hz]. Initial Rate (M/s) 0.10 0.20 0.0150 0.10 0.30 0.0225 0.20 0.20 0.0600 The numerical value of the rate constant is: (what are the units?) a. 380 b. 0.75 c. 7.5 d. 3.0 x 10-3
over the 11. In the reaction CLC) + 3F18) -- 2 CIF), if the average rate first 6.00 s, how much CIF, will form during this time S 2CFL the d ance of F, Fis 0250 -0.250 0.750 M b. 1.00 d. 2.00 M 1.50 M 3.00 M 12. Given the following data in the der of the reaction with respe 2 NO(g) ) - 2 NOCIS) Experiment INOT (M) 0.0300 0.0150 ICI (M) 0.0100 0.0100 0.0-400 Rate (M )...
Lab Questions 1. Use the Method of Initial Rates to determine the complete rate law for the reaction: 2 NOg)+ H2(g)-> N24g) +2 H20g) Trial [H2] 0.0100 0.0200 0.0300 0.0100 0.0100 NO Initial Rate, M/s 3.82 x 10- 7.63 x 103 1.14 x 102 1.53 x 102 3.43 x 102 20.0100 2 00100 30.0100 0.0200 0.0300 4
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