Following data is obtained in a chemical reaction occurring with a single reactant. The order of the reaction will be if t1/2 = 40 min; %3D t3/4=360 min 9. EO forCu2+ (aq.) + e Cu+ (aq) and Cu+ (aq.) + e Cu (s) are respectively are +0.15 and 0.50 V. Then ECU2+/CuO will be 0.15 V O 0.5 V 0.325 V 0.65 V
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- The following results were found after completion of Part C in the Experimental procedure: 0.056 M I- and 0.048 M H2O2 were used Run Catalyst Calculated Rate of Reaction (M/s) 1 none 0.031 2 10.00mL of 0.35 M FeCl2 0.52 Assuming the Rate Law = k[I-][H2O2] 2 Calculate the value of k for run 2. Give your answer to the nearest whole number.Determine the average rate of change of BB from ?=0 st=0 s to ?=272 s.t=272 s. A⟶2BA⟶2B Time (s) Concentration of A (M) 0 0.7300.730 136136 0.4450.445 272272 0.1600.160 rateB= __________M/sA general reaction written as A + 2B ® C + 2D is studied and yields the following data: [A]0 [B]0 Initial D[C]/Dt 0.150 M 0.150 M 8.00 ´ 10-3 mol/L·s 0.150 M 0.300 M 1.60 ´ 10-2 mol/L·s 0.300 M 0.150 M 3.20 ´ 10-2 mol/L·s Determine the initial rate of consumption ([deltaB]/delta t) for the first trial:
- In a batch reactor, reactant A is steadily converted into product B. The initialconcentration of reactant A is 100 mg/L. During a 10-hour reaction course, it wasobserved that the concentration of A in the reactor decreased at a constant rate of 10mg/L per hour. Based on the result, you can determine that the transformation reactionA→B follows ( ) with respect to reactant A.The peroxydisulfate ion (S2O8-2) reacts with the iodide ion in aqueous solution via the reaction: S2O82-(aq) + 3I- → 2SO4(aq)+ I3-(aq). An aqueous solution containing 0.050 M of S2O8-2 ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. Time (s) 0.00 400.0 800.0 1200.0 1600.0 [I‑] (M) 0.072 0.057 0.046 0.037 0.029 Determine the concentration of S2O82- remaining at 400 s in M. Determine the concentration of S2O82- remaining at 800 s in M. Determine the concentration of S2O82- remaining at 1600 s in M.The peroxydisulfate ion (S2O8-2) reacts with the iodide ion in aqueous solution via the reaction: S2O82-(aq) + 3I- → 2SO4(aq)+ I3-(aq). An aqueous solution containing 0.050 M of S2O8-2 ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. Time (s) 0.00 400.0 800.0 1200.0 1600.0 [I‑] (M) 0.072 0.057 0.046 0.037 0.029 Determine the average rate of disappearance of I- between 400.0 s and 800.0 s in M/s. Determine the average rate of disappearance of I- in the initial 400.0 s in M/s. Determine the average rate of disappearance of I- between 1200.0 s and 1600.0 s in M/s. Determine the concentration of S2O82- remaining at 400 s in M. Determine the concentration of S2O82- remaining at 800 s in M. Determine the concentration of S2O82- remaining at 1600 s in M.
- 2. In the reaction, R→P, a run with [R]0 =2.571M, [R] is found to be 2.361M at t=59.0s. A run with [R]0 =3.137M, [R] is found to be 2.439 M at t = 1.8 min. How much R will be consumed if a run with [R]0 = 0.501 M is allowed to form P for t = 4.0 min. Express your answer in 2 DPs.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)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=
- 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.Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.340 0.210 0.0204 2 0.340 0.420 0.0204 3 0.680 0.210 0.0816 ?=The following results were found after following the procedure Part B in the experiment: 0.053 M I- and 0.041 M H2O2 were used Temperature (oC) Calculated Reaction Rate (M/s) 12 0.031 30 0.119 88 0.797 Assuming the Rate Law = k[I-]2[H2O2] 2 Calculate the value of k at temperature 88oC. Give your answer to 1 place after the decimal.