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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+]
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- Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.A +B - C [A](M)[B](M) Initial Rate (M/h) 0.106 0.137 200 0.540 0.137 727 0.106 0.508 1,488 Find the order with respect to B. Round to the nearest whole number.A+B-C A(M) B(M)Initial Rate (M/h) 0.154 0.189 163 0.684 0.189 726 0.154 0.809 892 Find the order with respect to A. Round to the nearest whole number.
- A +B - C [AJ(M)[B](M) Initial Rate (M/h) 0.153 0.191 122 Using the rate equation Rate k[A]™[B]", and the partial data table above, find k if m=1 and n=1. Please do not include units.NH4+ {aq) + NO2(aq) -> N2(g) +2H2O{l} Data Initial [NH4+] Initial [NO2-] rate 1 0.0100 0.200 5.4 x10-7 2 0.0200 0.200 10.8x10-7 3 0.0400 0.200 21.5x10-7 4 0.200 0.0202 10.8x10-7 5 0.200 0.0404 21.6x10-7 6 0.200 0.0808 43.3x10-7 Find x,y,k2. Consider the kinetic data of the reaction of P + 2 Q + 2+ - PQ, + Z*and answer the succeeding questions: Experiment P (M) Q (M) Temp ("C) Initial Rate, M/s 1 0.01150 0.01200 0.00000 25 4.80 x 10-4 2 0.02300 0.01200 0.00000 25 1.92 x 10-3 3 0.01150 0.02400 0.00000 25 9.60 x 10-4 4 0.04600 0.01200 0.00000 25 7.68 x 10-3 5 0.01150 0.04800 0.00000 25 1.92 x 10-3 6 0.01150 0.01200 0.00000 10 5.10 x 10-5 0.01150 0.01200 0.00000 40 4.55 x 10-3 0.01150 0.01200 0.00500 10 4.98 x 10-5 0.01150 0.01200 0.01050 25 4.82 x 104 10 0.01150 0.01200 0.02100 40 4.44 x 10-3 A. Determine the rate order with respect to P. Determine the rate order with respect to Q. C. Determine the rate law of the reaction. What is the average rate constant? Indicate the appropriate units. E. What is the energy of activation and frequency factor of the reaction without the additive ion? Include the equation of the best fit line of the Arrhenius equation and RSQ Note: Use the calculated rate constant in set up 1 for 25°C…
- the mean time, the rate, [S₂O3] in the reaction may label clear outliers the mean) as such and e calculation. on mixtures NH4)2SO4 (NH4)2S2O8| (mL) (mL) 1.50 0.50 1.50 0.50 1.00 1.00 1.00 1.00 following reagents are um iodide ium persulfate m thiosulfate um nitrate ium sulfate odide in the solution in the Answer: 0.050 M • Determination of the rate law follows the protocol in ref. (5). with one difference. A reactant order (rate law exponent) will be calculated twice using two different pairs of determinations (e.g. determinations 1 & 2 and determinations 3 & 4). Then the mean is taken of both values and reported as order. This is done for each reactant. This additional step allows us to include more data and reduce experimental error. Practice Problem 2: The rate of a reaction CO(g) +3H₂(g)→ CH4(g) + H₂O(g) was determined at 25 °C. From the following data, determine a) the mean reaction order with respect to CO b) the mean reaction order with respect to H₂ c) the overall rate order d)…Determine the average rate of change of B from t = 0 s to Time (s) Concentration of A (M) t = 352 s. 0.760 176 0.450 A 2 B 352 0.140 rateB = M/s - TOOLS x10 NOV 1 étv MacBook Air 80 DII DD F4 F5 F6 F7 F8 F9 F10 F11 F12 %23 & *1. A → B +B (rate constant = k1) 2. A +B → C+D (rate constant = k2 3. D → E+F (rate constant = k3) 4. F+A → D + G (rate constant = k Express the net change of [F] and [G]& (select 2 answers) а. d[F] = -k3[D]+k4[A][F] dt b. d[G] = -k4[A][F] dt d[E] = -k3[D] dt d[F] = k3[D]-k4[A][F] С. dt d. d[F] = k3[E][F]-k4[A][F] dt = k4[A][F] dt е. d[E] = k3[D] dt f. d[G] = k4[D][G] %3D dt d[E] = k3[E][F] dt
- 1-arr In a study of the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N2O5- →2 NO2 + ½ O2 the concentration of N,O5 was followed as a function of time. It was found that a graph of In[N2O5] versus time in minutes gave a straight line with a slope of -6.31×10* min and a y- intercept of -1.34 . Based on this plot, the reaction O order in N,0g and the rate constant for the reaction is min-1. zero first secondDetermine the average rate of change of B from t = 0 s to Time (s) Concentration of A (M) t = 352 s. 0.760 176 0.450 A → 2 B 352 0.140 rateg = M/s TOOLS x10 NOV étv 1 MacBook Air 80 888 DII DD F12 F3 F9 F10 F11 F4 F5 F6 F7 F8A +B - C [AJ(M) B](M) Initial Rate (M/h) 0.213 0.144 117 0.302 0.144 355 0.213 0.353 541 Find the order with respect to A.