Thermodynamics 6.2. Multiple components (1.5 pt) Assume we have a reaction with the following stoichiometry In...
For a hypothetical chemical reaction that has the stoichiometry 2X + Y -----Z the following initial data were obtained X (Mol/L Y(Mol/L) rate of formation of Z (Mol/L s .4 .2 1.4 x 10^-3 .4 .4 2.8 x 10^-3 .2 .1 7.0 x 10^-4 .6 .6 4.2 x 10^-3 Give rate Law for this reaction Callculate rate constant and specify units How long must reaction proceed to produce concentration of Z =to .2 molar if initial concentrations of x=.8M and...
Question 2 For an isothermal, constant volume batch reactor in which the following reaction is occurring A - B A laboratory technician measures the rate of reaction of A in a reactor for different concentrations, and obtains the following data: CA 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 1.0 [mol.L' -TA 0.1 0.4 0.9 1.6 2.5 3.6 4.9 6.4 10 (mol.L-min'] The laboratory technician tells you that if you plot - r against (CA) that you get a straight...
1) The following experimental data were obtained for a particular irreversible reaction at T = 25.0 °C. It is assumed that the reaction obeys a rate law of the form rate = - d[A]/dt = k [A]P [B]" (1.1) Trial [A]initial (mol/L) [B]initial (mol/L) (Rate) initial (mol/L•min) 0.00100 0.00100 0.00100 0.00100 0.00100 0.00200 0.00400 0.01000 2.6 x 10-8 1.2 x 10-7 3.9 x 10-7 2.4 x 10-6 0.00200 0.00400 0.01000 0.00200 0.00200 0.00200 1.5 x 10-7 1.1 x 107 1.6...
7. What is the reaction order for each reactant and the rate coefficient for the following reaction? A+B+C ->Z [A] (mol L B (mol L[C] (mol L ](mol L sec1) 0.010 0.020 0.010 0.020 0.0100 0.0100 0.0200 0.0100 0.10 0.10 0.10 0.20 3.0 x 10-2 3.0 x 102 1.2 x 10-1 1.5 x 10-2
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 →...
Please answer all, I rate, thank you. THE IODINE CLOCK- REACTION KINETICS EXPERIMENT 3 PRE-LABORATORY QUESTIONS (WEEK 1) Fully answer these questions in your laboratory notebook before coming to lab. Show all work for numerical calculations. 1. If the rate law for a reaction is Rate [A][B What is the overall order of the reaction? a. b. If the concentration of A is doubled and the concentration of B is tripled, how will this affect the rate of the 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...
The kinetics of the following reaction have been studied: 4 NO + O2 → 2 N2O3 The rate of appearance of N2O3 was measured as ∆[N2O3]/∆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 ∆[NO]/∆t in mol L-1 s-1? (c) What is ∆[O2]/∆t in mol L-1 s-1?
Homework 8-3_1 Reaction Rate Orders, Temp Effects Reaction Rates and Rate Orders The following initial rate data was collected for the reaction: HI(g) + CHşl(g) à CH.(g) +1-(9) Experiment (HI) (CHI) Initial Rate 0.015 M0.900 M 4.01 x 10M's 0.030 M0.900 M 8.04 x 10'Ms 0.030 M0.450 M 3.99 x 10 m/s 1. What is the rate law for this reaction? a. Rate =k [HI] [CHI] b. Rate = k [HI] [C,H,I] c. Rate = k [HI] (C,H,I] d. Rate...
Problem #3 (20 marks) The following kinetic data (initial rates) were obtained for the reaction 2 ICI(g) + H2(g) → 12(g) + 2 HCI (9) Experiment [Cl]. (mmol/L) [Hz]. (mmol/L) V. (mol/L s) 3.0 3.0 14.8 X10-7 3.0 1.8 8.9 x10-7 1.5 1.8 4.44 x 10-7 3.7 1.3 ? (a) Write the rate law for the reaction (b) From the data, determine the value of the rate constant (c) Use the data to predict the reaction rate for experiment 4.