Reaction Order and Rate Law Essay

July 18, 2017 Law

Data. Calculations. and Questions

A. Calculate the initial and concluding concentrations as needed to finish Tables 1 and 2.

Data Table 1: Changing the Concentration of 1. 0 M HCl

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| | | | |Concentrations | | | # Drops | # Drops | # Drops |Initial |

| # Drops | # Drops | # Drops |Initial |Initial |Final |Final |Reaction Time ( sec ) |Reaction | |Well # |HCl |Water |Na2S2O3 |HCl |Na2S2O3 |HCl |Na2S2O3 |Trial 1 |Trial 2 |Avg |Rate ( sec-1 ) | |1 |8 |0 |12 |1 M |0. 3 M |0. 4 |0. 18 |18. 4 |16. 3 |17. 35 |0. 0576 | |2 |8 |6 |6 |1 M |0. 15 |0. 4 |0. 0045 |37. 1 |37. 9 |37. 5 |0. 0267 | |3 |8 |8 |4 |1 M |0. 1 |0. 4 |0. 02 |107. 2 |106. 6 |106. 9 |0. 0093 | |

B. Calculate the mean reaction clip for each reaction by adding the times for the two tests and spliting by 2.

C. Calculate the reaction rate by taking the opposite of the mean reaction clip. i. e. . 1 divided by the mean reaction clip.

1. Use table 1 to find the reaction order for HCl.
2. Use table 2 to find the reaction order for Na2S2O3.

Remember. you want to see what happens to the reaction rate when you double the concentration of one reactant while the 2nd reactant remains unchanged. In Part 1. we varied the concentration of HCl while we kept the concentration of Na2S2O3 the same. In Part 2 we varied the concentration of Na2S2O3 while maintaining the concentration of HCl the same. These are experimental informations and consequences will be different from some of the nice. even Numberss you saw on text edition jobs. For illustration. in this experiment you may duplicate the concentration of a reactant but the reaction rate may increase anyplace from 1. 7 times to 2. 4 times. This still means an approximative doubling of the reaction rate. On the other manus. if you double a reactant concentration and the reaction rate additions by 0. 7 to 1. 3 times that likely means that the reaction rate multiplier is one ( 1 ) .

D. Write the rate jurisprudence for the reaction.

E. Using the rate jurisprudence. the rate. and the appropriate concentration ( s ) from one ( or more ) of your experiments calculate Ks.

F. What are the possible mistakes in this experiment?

———————–
Laura Titus

Done in the tabular array

Time average=time test 1+time test 2/2

HCl reaction is 1. 36

Na2S2O3 reaction is 0. 84

Rate jurisprudence = K [ HCl ] ^1. 36 [ Na2S2O3 ] ^0. 84

Rate law=k [ 0. 024 ] ^1. 36 [ 0. 0576 ] ^0. 84

Rate law= K [ . 03264 ] [ . 048384 ]

K=1/ . 00158

K= 632. 9?

Me non to the full certain if my Numberss are right or non. Rounding right. documenting at right clip.

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