Initial Concentrations (mol/L) Initial Rate I ClO OH (mol/(L · s)) Exp. 1 0.010
ID: 677349 • Letter: I
Question
InitialConcentrations (mol/L)
Initial Rate I ClO OH (mol/(L·s)) Exp. 1 0.010 0.020 0.010 1.22 10-1 Exp. 2 0.020 0.010 0.010 1.22 10-1 Exp. 3 0.010 0.010 0.010 6.1 10-2 Exp. 4 0.010 0.010 0.020 3.0 10-2 Iodide ion is oxidized to hypoiodite ion, IO?, byhypochlorite ion, ClO?, in basic solution. The equation isgiven below. The following initial-rate experiments were run and, for each, theinitial rate of formation of IO? was determined. Find therate law and the value of the rate constant. rate law rate =k[I - ][ClO- ]/[OH-] rate =k[I - ][ClO- ] rate =k[ClO- ]/[OH - ] rate =k[I - ][OH - ] value of rate constant 2 Top of Form units of rate constant Bottom of Form M2s-1 M -2s-1 M -1s-1 s-1 M s-1
Explanation / Answer
Initial Concentrations (mol/L) Initial Rate I ClO OH (mol/(L · s)) Exp. 1 0.010