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- 2. Compare the value you calculated with the actual value (-601.8 kJ/mol). Show your determination of percent error. Use the standard equation for this: actual value - experimental value %error = x 100% |actual value| ragraph* and which the & 3 4 7 8Reaction Conc. Na2S203 Conc. HCI A Abs. A Time (s) Rate (A Abs./BA Time) 1.3686611 1.5360817 1.2267196 1.007568 |0.300349 |0.01870913 |0.02870913 1 0.10 M .30 М 1.358380874 2 0.10 M .15 M 5.114311671 3 0.050 M .30 M 65.56796601 4 0.025 M .30 M 0.9563164 11.3085840 3. What is the overall order of the reaction? Write the complete rate law for this reaction.Reaction Conc. Na2S½O3 Conc. HCI A Abs. A Time (s) Rate (A Abs./ga Time) 1.007568 0.300349 0.01870913 0.02870913 1 0.10 M .30 М 1.3686611 1.358380874 0.10 M .15 M 1.5360817 5.114311671 3 0.050 M .30 M 1.2267196 65.56796601 4 0.025 M .30 M 0.9563164 11.3085840 4. Use experimental data and the rate law to calculate a rate constant for each reaction 1, 2, 3, 4. How do the rate constants compare? Should they be the same or different? Discuss in your conclusions. Report the average value of your calculations. Be sure to include units in your rate constant. The rate law of the reaction is shown below: Rate = [Na2S2O3]-2
- 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)…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.Please quickly ?❤️
- can someone please help with these?! will rate, ty in advanceWhat is the rate? lodine chloride reacts with hydrogen to produce iodine and hydrogen chloride. 2ICI + H2 --> 2HCI Trial ICI(mol/L) H2(mol/L) Initial rate mol/Ls 5.84 x 107 0.0015 8.76 x 10-7 0.0030 1.17 x 106 0.0060 0.20 2. .0.40 0.20 Include UnitsE=Eº OF O E° = RT nF RT nF E-nF E° = E RT nF ) Stry fes - સની ડિગ m B rate HITTETEAD fesses millesim
- Which energy levels precede and succeed 4s ?Ne(g) effuses at a rate that is ______ times that of Kr(g) under the same conditions. rateNe/rateKr=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