(2 points each a-f) The data below were collected for the following reaction: 2 NO2 (g)...
6. (20 pts) The data below were collected for the following reaction at 25 °C: NO2(g) + CO(g) ? NO(g) + CO2(g) [NO2Initial 0.100 M 0.200 M 0.200 M 0.400 M COJinitial 0.100 M 0.100 M 0.200 M 0.100 M Initial rate 0.0021 Ms 0.0082 Ms 0.0083 Ms 0.033 M s a. (8 pts) What is the rate law for this reaction? (in the form Rate k[NOJ'icoj) b. (6 pts) What is the value of K? (Be careful with units...
For the reaction 3A(g) + 2B(g) → 2C(g) + 2D(g) the following data was collected at constant temperature. Determine the correct rate law for this reaction. Trial Initial [A]mol/L Initial[B]mol/L Initial Rate 1 0.200 0.100 6.00*10^-2 2 0.100 0.100 1.50 *10^-2 3 0.200 0.200 1.20*10^-1 4 0.300 0.200 ???????? Predict the rate of the reaction for Trial #4
Reaction Equation: NO2 (g) + CO(g) ⟶ NO(g) + CO2 (g) Experiment Number Inital concentration of [NO2] (M) Inital concentration of [CO] (M) Initial rate (M/s) 1 0.200 0.200 5.00X10-4 2 0.200 0.800 8.00X10-3 3 0.600 0.200 5.00X10-4 A.) Determine the order (0, 1, or 2) with respect to NO2. B.) Determine the order (0, 1, or 2) with respect to CO.
2. The following data were measured for the reaction BF3 (g)+NH, (g) FBNH (g): Experiment 0.250 0.250 0.200 0.350 0.175 NH,J (M) 0.250 0.125 0.100 0.100 0.100 Initial Rate (M/s) 0.2130 0.1065 0.0682 0.1193 0.0596 4 a. b. c. What is the order of this reaction with respect to each reactant? What is the rate constant, with proper units, for this reaction? What is the rate law for this reaction?
Consider the reaction: 2 NO(g) + O2 (g)--> 2 NO2 (g) The following data were obtained from three experiments using the method of initial rates: 3. Consider the reaction: 2 NO(g) + O2(g) → 2 NO2(g) The following data were obtained from three experiments using the method of initial rates: Initial [NO] Initial rate NO Initial [02] mol mol L-1 mol L-1 L-15-1 0.010 0.010 Experiment 1 Experiment 2 Experiment 3 0.020 0.010 2.5 x 10-5 1.0 x 10-4 5.0...
For the reaction 3A(g) + 2B(g) → 2C(g) + 2D(g) the following data was collected at constant temperature. Determine the correct rate law for this reaction and value of rate constant. Trial Initial [A] Initial [B] Initial Rate (mol/L) (mol/L) (mol/(L• min)) 1 0.200 0.200 1.20 × 10–1 2 0.200 0.100 6.00 × 10–2 3 0.100 0.200 3.00 × 10–2 Predict the rate of reaction for Trial #4 using the correct rate law and rate constant. 4 0.300 0.200 ?????????
1a. The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g) The reaction is second order with respect to NO(g) and first order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.6 x 102 M–2 s–1. When the initial concentrations of NO and O2 are 0.02 M and 0.015 M, respectively, the rate of the reaction is ___ M/s. 1b. The rate constant of a first-order decomposition reaction is 0.014...
8) The rate law for the following reaction N2O(g) + NO2(g) → 3NO(g) is Rate = k [N2O][NO2]2. Fill in the blank in the table below. Experiment [N2O], M [NO2], M Initial Rate, MS-1 1 0.100 0.100 2.0x10-3 2 0.300 0.100 6.0x10-3 3 0.100 0.200 ? a) 2.0x10−3 Ms−1 b) 4.0x10−3 Ms−1 c) 8.0x10−3 Ms−1 d) 6.0x10-3 Ms-1 e) 1.0x10−2 Ms−1
The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g) The reaction is second-order with respect to NO(g) and first-order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.7E+2 M–2s–1. What is the rate of reaction when the initial concentrations of NO and O2 are 1.95E-2 M and 1.40E-2 M, respectively? 5.32E-6 M/s 2.50E-3 M/s 1.80E-3 M/s 0.128 M/s -2.50E-3 M/s
3. For the reaction C3H3(g) + 5 O2(g) ----> 3 CO2(g) + 4H20(1) the following rate data were determined at 30°C. Experiment Initial C3H8 Initial O2 id. Rate 0.200M 0.200 M 3.00 x 101 0.400 M 0.200 M 6.00 x 101 0.200 MO 0.400 M 1 .20 x 102 a) Determine the reaction order with respect to C3H8. b) Determine the reaction order with respect to 02. c) Calculate the rate constant at this temperature. d) Write the rate law...