Calculate the reaction rate for each trial using an average of the time (in sec) for each trial

Chemistry How can I find the rate orders.

Pure A and B are mixed together at the same concentration of 0.361 M. After 7.00 minutes, the concentration of A is found to be 0.048 M. Find the average rate with respect to A.

Using the data in the table, calculate the rate constant of this reaction.   A+B⟶C+D   Trial [?] (?) [?] (?)[) Rate (M/s) 1 0.370 0.390 0.0234 2 0.370 0.936 0.135 3 0.592 0.390 0.0374 ?= ?    units= ?

integrated rate law plot for reactant A with time would give you a linear fit? 8) Given the experimental data below, determine the rate law and rate constant (with units) of the reaction. Which Trial [A], M [B], M Initial Rate, M.s1 1 0.10 0.10 0.0019 234 0.20 0.10 0.0081 0.20 0.20 0.0084 0.40 0.30 0.033 Rate Law: Rate Constant: Integrated rate law plot:

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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)…

Rank the following in order of increasing rate in a unimolecular reaction. (1=slowest ... 3=fastest)

Based on the information in the data table and your graph, explain the relationship between percent concentration of catalase and rate of reaction.   Did your actual results match your hypotheses? If not, why?   my hypothesis If increase the concentration of the reactant, there will be more of the chemical reactant. More reactant particles moving together permit more collisions to happen and so the response rate is expanded. The higher the concentration of reactants, the speedier the rate of a response will be.

1. Experimental data: [A]               [B]                   Rate (M/min) 0.015.         0.015               2.95 0.025          0.015               5.61 0.015          0.025               5.82 a. What is the Rate Law (calculate the orders to 2 decimals)? b. Calculate the Rate Law Constant (use the rounded-off orders & experiment 1). c. Calculate the rate (use the rounded-off orders) when [A] = .150 M and [B] = .550 M