Question 3 Consider the set of elementary reactions k₁ A B k2 A + B C k3 A+D 2E At time t = 0, a batch reactor is filled with a mixture of A and D. What is the relation between the concentration of B and D after a time t? O CD= (K1-K₂ CB)(k2/k3) O CD= (K₁-K2 CB)(k1/k2) NOTG O Cp (K₁-K₂ CB)(k3/k2)
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- 2. Consider a gas-phase reaction: A + 2B → C that takes place in a packed-bed reactor (PBR) with a catalyst volume of 0.2 L. The feed rate of A is 0.1 mol/s and the feed rate of B is 0.2 mol/s. The reaction rate constant is 0.01 L/(mol*s) and the pressure drop across the catalyst bed is 2 bar. What is the conversion of A at the exit of the reactor?Reducing NO Emissions Adding NH3 to the stack gases at an electric power generating plant can reduceNOx emissions. This selective noncatalytic reduction (SNR) process depends on the reaction between NH3 (an odd-electron compound) and NO.$$4NH3(g)+6NO(g)5N2(g)+6H2O(g)The following kinetic data were collected at 1200 K. Experiment [NH3] (M) [NO] (M) Rate (M/s) 1 1.00x10-5 1.00x10-5 0.120 2 2.00x10-5 1.00x10-5 0.240 3 2.00x10-5 1.50x10-5 0.360 4 2.50x10-5 1.50x10-5 0.450 What is the rate-law expression for the reaction? Do not add multiplication symbols to your answer. $$Rate=Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.310 0.370 0.0139 2 0.310 0.740 0.0139 3 0.620 0.370 0.0556 Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D ?= Units:
- The gas phase reaction A→B+2C is carried out in a constant volume batch reactor (V=25 L). Twenty moles of A with 80% purity (the remainder is inert) are introduced into the reactor.Calculate the time to reduce the concentration of A to 0.1 mol/L if the reaction is first order with k=0.524 min-1.Calculate the time required to consume 10 mols of A if the reaction is second order and k=0.982 L/mol.h.If the temperature is 150°C, what is the total initial pressure? What is the final total pressure if the reaction occurs in its entirety? Explain why pressure varies in this situation.Trial 0.010 M [NaOH] 0.10M [CH3COOC2H5] Initial conductivity of NaOH solution (uS/cm) Initial rate (uS/cm)/s) 1 21.0ml 2.1 ml 1285 24.72 2 21.0 ml 2.1 ml 2399 50.32 3 21.0 ml 2.1 ml 1262 23.72 What is the order of the reaction in sodium hydroxide and ethyl acetate? Explain how you determined order for each reactant.Examine the experimental data shown in the table below for the following reaction: (make sure to show your work for each part) A + 5B + 6C ---> 3D + 3E Experiment [A] (M) [B] (M) [C] (M) Rate (M/s) 1 0.35 0.35 0.35 8.0 x 10-4 2 0.70 0.35 0.35 3.2 x 10-3 3 0.70 0.70 0.35 6.4 x 10-3 4 0.70 0.35 0.70 3.2 x 10-3 A. What is the reaction order of A? B. What is the reaction order of B? C. What is the overall rate equation for this reaction? D. What is the value of the rate constant? E. What are the units of the rate constant?
- Given Zn(s)| Zn 2+ (aq) (1M) || Ag+2+ (aq) (1M) | Ag (s) Eocell = 1.562V What will the Ecell be if the [Zn2+] = 0.75M and [Ag+] =0.25 M at 40.00oC (313.15K)? The overall reaction is Zn(s) + 2 Ag+ (aq) --> 2 Ag (s) + Zn 2+ (aq) (Answer has 3 digits after the decimal)In Experiment 4- Chemical Kinetics “The Rate of Chemical Reaction”, the following data were obtained: Rxn Mixture time(s) temperature (˚C) 1 190 23.0 2 378 23.0 3 97 23.0 4 205 23.0 5 44 23.0 6 90 35.0 Concentrations and portions for reaction mixture number one: H2O 0.050 M Buffer 0.050 M KI (mL) 0.1% Starch (mL) 0.0450 MNa2S2O3(mL) 0.8525 M H202 (mL) 75.0mL 30.0mL 25.0 5.00 5.00 10.00 Use the data above to answer the following questions where applicable. (a) Write the formulas of the reactants, there are three, in the reaction being studied.Signs + or - or subscripts may be entered all on the same line; S2O32- can be entered as S2O3^2-, the symbol, ^, is not required if the…2I– (aq) + H2O2 (aq) + 2H3O + (aq) → I2 (aq) + 4H2O (l) (slow) C6H8O6 (aq) + 2H2O (l) + I2 (aq) → C6H6O6 (aq) + 2H3O + (aq) + 2I– (aq) (very fast) I2 (aq) + I– (aq) ⇌ I – 3 (aq) I3- (aq) + starch → blue I3- · starch complex (aq) (fast) A different 0.100 L reaction mixture is prepared with initial concentrations of 1.0×10−2 M iodide I– , 2.0 × 10−3 M ascorbic acid C6H8O6 , and 0.135 M hydrogen peroxide H2O2 . If the first two reactions above procede at the same rate (they’re limited by the first one!), which of these reactants will be completely consumed first?
- Use the following data to calculate the reaction rate law and the rate law constant for the system. ??(?)+?2(?)→???2(?) Trial Run [NO] (mol/L) [H2] (mol/L) Initial Rate (mol/L∙s) 1 0.001 0.004 0.002 2 0.002 0.004 0.008 3 . 0.003 0.004 0.018 4 0.004 0.001 0.008 5 0.004 0.002 0.016 6 . 0.004 0.003 0.024 a) rate = k[NO][H2]2, where k = 7 L2/mol2∙s b) rate = k[NO]2[H2], where k = 5.0x105 L2/mol2∙s c) rate = k[NO][H2], where k = 5.0x105 L2/mol∙s d) rate = k[NO]2[H2]3, where k = 3.0x10-7 L/mol2∙sQ.4a) What the rate order with respect to the water? Notetreat the volume the water [10mL = 10M] and [20mL = 20N] We can evaluate these assumptions based on the fact we're only attempting ascertan orders that are directly proportion to their respective volumes in case.b.) What is the rate order with respect to the Buffer ? Question-5: Write the correct rate larw expression for the reaction? Question-6: Choose reaction-1 and give the rate law constant k for trial-1.Determine the rate law, rate constant(k) of the reaction with the given information. What's the balanced reaction using the half-reaction method. Also for experiment 1 what will be the concentration of [Fe2+] after 10 seconds? Chart Shows the initial reaction rate measurement for the acidic conditions performed in acidic condition (H+). Equation 2Fe2+(aq)+Cl2(aq)----> 2Fe3+(aq)+2Cl-(aq) Experiments [Fe2+] [Cl2] [H+] Rate Experiment 1 0.0014 M 0.0045 M 0.10 M 1.03x10-5 M/s Experiment 2 0.0040 M 0.0045 M 0.10 M 1.98x10-5 M/s Experiment 3 0.0014 M 0.0090 M 0.10 M 2.02x10-5 M/s Experiment 4 0.0040 M 0.0090 M 0.10 M 3.90x10-5 M/s Experiment 5 0.0014 M 0.0045 M 0.05 M 1.97x10-5 M/s Experiment 6 0.0014 M 0.0045 M 0.01 M 9.98x10-5 M/s