1) Use Table 1 to determine the reaction order for HCl 2) Use Table 2 to determi
ID: 984223 • Letter: 1
Question
1) Use Table 1 to determine the reaction order for HCl
2) Use Table 2 to determine the reaction order for Na2S2O3
3) Write the rate law for the reaction
4)Using the rate Law, the rate, and the appropriate concentrations from one or more of the experiments calculate k
Experimental Data and Calculations Data Table 1 Varying the Concentration of 1.0 MHCl Concentrations- #of #of! #of ! Initial Initial Final | Final | Reaction Time (sec) | Reactio Drop Drop Drops WelHCI Wate Na2S2OHCl NaS20 HCl Na2S2O Trial Tria Averag Rate 12 e 12M44.0 42.5743.32 0231 sec 12 0 1M 0.3M 6M 0.5M 0.3M .3M21M 47.5 55.75 51.64 .0194 4 0.33 0.3M .19824M 55.0 71.11 63.0 .0159 Data Table 2 Varying the Concentration of 0.3 M Na2S2Os -Concentrations-- #of! #of #of!Initia Initial Fina Final Drop Drop Drops Reaction Time (sec) | React. WelHCI Wate Na2S2O HC Na2S20 HCl Na S20 Trial Tria Average Rate (sec1) 1M 0.3M 4M 18M 33.84 30.4 32.13.0311 0 12 1M 0.15M .7M .09M 72.9059.38 66.14 .0151 1M 0.1M 8M 06M 124.9 97.22 111.00090 4 4Explanation / Answer
1) To determine th reaction order for HCl we see how is the variation in the rate when we change the concentration in HCl.
when we have 1M the rate is 0.0231,
when we divided the contretion into a half 0.5 M the rates is 0.194
so if we divide 1/0.5= 2 and 0.0231/0.0194 = 1,19
and if we divid 1/0,33= 3 and 0.0231/0.0159= 1,45
Then the rate of the reaction does not depend on the concentration of the HCl. So the reaction order is 0 for HCl
2) We do the same calculations for the data given in the table and we observe that when we have the half of the concentration the rate decreases in a relation of 2, and when we decreases the concentration to a 3rd part the relation of the rates decreases in 3.
So the order of the reaction for the Na2S2O3 is 1.
3) the rate law for the reaction will be in first order only dependin on the Na2S2O3 concentracion
k= [Na2S2O3]
4) to find the rate law you need to do a plt of [Na2S2O3 ] Vs reaction rate of the table 2 and you wil obtain a straight line, then you can calculate the k from the equation
reaction rate = k [[Na2S2O3 ]
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