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- For the given equation at 600 oC:CO(g) + Cl2(g) à COCl2(g), the following data were collected: Experiment[CO] (M)[Cl2] (M)Rate of appearance COCl2 (M/s) 1 0.24 0.400.121 2 0.48 0.400.241 3 0.24 0.800.483 Determine the Rate Law and the value of the Rate constant (with appropriate units).Please check! 1.Determine the overall reaction order for the reaction, A+B→2C using the table of data below: Experiment Initial [A]/M Initial [B]/M Initial rate/M s-1 1 0.010 0.040 0.0031 2 0.010 0.020 0.0015 3 0.020 0.020 0.0032 a. 0 b. 1 c. 2 <-- I think it's this one b/c the numbers are doubled in the table. d. 3 2. The overall order for the reaction, A+B→C, is 2. A student tests this by measuring the reaction rate at one concentration of A and B, then doubling both concentrations at the same time and re-measuring the rate, which quadrupled. The student concludes that the data support the hypothesis that the above rate law is rate=k[A][B]. Analyze this. a. The data do support the hypothesis but each trial should be repeated. b. The data contradict the hypothesis because the rate should have doubled, not quadrupled. <-- c. The data support the hypothesis but a trial holding one reactant constant is needed. b. The data contradict the hypothesis but testing by…Consider the following potential-energy curves for two different reactions: a. Which reaction has a higher activation energy for the forward reaction? b. If both reactions were run at the same temperature and have the same orientation requirements to react, which one would have the larger rate constant? c. Are these reactions exothermic or endothermic?
- Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO2(aq) + 2OH–(aq) → ClO2–(aq) + ClO3–(aq) + H2O A kinetic study of this reaction under a certain set of conditions yielded the data below. Experiment [ClO2] (M) [OH-] (M) Rate (M/s) 1 0.0500 0.100 5.75 x 10-2 2 0.100 0.100 2.30 x 10-1 3 0.100 0.0500 1.15 x 10-1 What is the rate law?Experiment Initial [Br–] (M) Initial [BrO3–] (M) Initial [H+] (M) Rate of Disappearance of BrO3– (M s-1) 1 0.00100 0.00500 0.100 2.50x10-4 2 0.00200 0.00500 0.100 5.00x10-4 3 0.00100 0.00750 0.100 3.75x10-4 4 0.00100 0.01500 0.200 3.00x10-3 Determine the order of the reaction for [H+]For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate(M/s) 1 0.50 0.50 0.50 1.5×10−4 2 0.50 0.50 1.50 4.5×10−4 3 1.00 0.50 0.50 6.0×10−4 4 1.00 1.00 0.50 6.0×10−4 What is the value of the rate constant k for this reaction?
- 21. What is ∆H (in kJ/mol) for a reaction where the activation energy is 250 kJ/mol while the activation energy for the reverse reaction is 125.0 kJ/mol? 23. The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 × 10⁻⁴ s⁻¹ at 311 K, what is the rate constant at 273 K? 24. An experimental plot of ln(k) vs. 1/T is obtained in lab for a reaction. The slope of the best-fit line for the graph is -3005 K. What is the value of the activation energy for the reaction in kJ/mol?The initial rate of the reaction between AA and BB was measured. From the data given,a. determine the order of each reactant,b. determine the order of the reaction,c. write the rate law andd. calculate the rate constant, k. Experiment A B initial rate #1 0.20M 0.10M 3.50x10-3M/s #2 0.40M 0.10M 7.00x10-3M/s #3 0.40M 0.40M 7.00x10-3M/s if a reaction is second order in B and the concentration of B increased from 0.0850M to 0.2975M, what should happen to the rate?We have the reaction 2A + 2B + C → D + 3E A plot of Ln (pressure in torr) versus 1/ T (in kelvin) produce a straight line with an equation of the line Y=-23.70X+ 1.56 In addition, the following data were obtained: Experiment [A] (M) [B] (M) [C] (M) Initial rate (M.s-1) 1 0.024 0.085 0.032 6.0×10-6 2 0.096 0.085 0.032 9.6×10-5 3 0.024 0.085 0.080 1.5×10-5 4 0.024 0.170 0.032 1.5×10-6 Determine the ∆H for this reaction in (kJ/mol) and determine if the reaction is exothermic or endothermic.
- The reaction, A → products, is known to be second order with respect to the concentration of A and second order overall. The rate constant for the reaction is 0.0225 M-1·min-1 at a certain temperature.If the initial concentration of A is 1.250 M. What will be the concentration of A after 108.0 min?Answer___ MHow long would it take for 90.0% of the starting material (A) to undergo reaction?Answer ___ minA chemical reaction has a rate constant value of 15.8 M-1·hr-1 at 175.0°C and an activation energy of 55.0 kJ/mol. How many degrees Celsius must the temperature be increased in order for the reaction rate to increase by a factor of 5.0?Answer °C increase in temperatureFor the reaction 2 NO(g) + O 2 (g) → 2 NO2 (g) have the following data. Experiment 1 2 3: [NO], M 0.010: 0.020: 0.010 [O 2 ], M 0.010 :0.010: 0.020 The speed of consumption of 2.5 x 10-5 1.0 x 10-4 5.0 x 10-5 NO, Ms -1 a) write the rate equation for the reaction b) calculate the rate constant