Consider the following reaction between mercury(II) chloride and oxalate ion. 2

Question

Consider the following reaction between mercury(II) chloride and oxalate ion. 2 HgCI2(aq) + C2O42-(aq) rightarrow 2 Cl -(aq) + 2 CO2(g) + Hg2CI2(s) The initial rate of this reaction was determined for several concentrations of HgCI2 and C2O42-, and the following rate data were obtained for the rate of disappearance of C2O42-. What is the rate law for this reaction? k[HgCI2]2[C2O4-2] k[HgCI2]-2[C204-2]1/2 k[HgCI2][C2O4-2]2 What is the value of the rate constant? M-2s-1 What is the reaction rate when the concentration of HgCI2 is 0.17 M and that of C2O4- is 0.11 M if the temperature is the same as that used to obtain the data shown above? M/s

Explanation / Answer

c d^2x/dt = 1.02 dx/dt = 3.5

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