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# rate of reaction

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1.

Step 1: Cl2 ------ 2Cl (fast)
Step 2: CHCl3 + Cl -------- CCl3 + HCl (slow)
Step 3: CCl3 + Cl ------------CCl4 (fast)

Identify the rate determining step, reaction intermediates and the experimental rate law (intermediates can not be in the rate law)

2. For the half-reaction

XeF2(aq) + 2H(+1)(aq) + 2e- ----------- Xe(g) + 2HF(aq) E(little circle) = +2.64

a). calculate the (triange)G for the reaction
XeF2(a) + H2(g)-------------Xe(g) + 2HF(aq)

b). given that the free energy of formation, (triangle)Gf(little circle), of HF(aq) is -276KJ/mol calcuate (triange)Gf fo XeF2(aq)

3. Acidic MnO4(-1) solution reacts with ethanol, CH3CH2OH, to produce acetic acid, CH3COOH.

a). Write a balanced equation for the reaction

b). What is the volume of 0.200 M MnO4(-1) solution is needed to titrate 22.5ml of a 0.350M solution fo ethanol.

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#### Solution Summary

Chemical reactions are investigated, such as rate and energy.

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## Lab Report: Reaction Order and Rate Laws

Objective: To study the effect of reactant concentration on the rate of the reaction between sodium thiosulfate and hydrochloric acid and to determine the order of each reactant and the rate law for the reaction.

2 HCI(aq) + NaS2O3 (aq) --> S(s) + SO2 (aq) + H2O(l) + 2NaCL(aq)

Calculations:

(a) Calculate the initial and final concentrations as needed to complete tables 1 and 2.
(b) Calculate the average reaction time for each reaction by adding the times for the two trials and dividing by 2.
(c) Calculate the reaction rate by taking the inverse of the average reaction time.
(d) Write the rate law for the reaction.

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