14.34 (a)
The reaction given is
2 ClO2 (aq) + 2 OH- (aq) --------> ClO3- (aq) + ClO2- (aq) + H2O (l)
Since the rate law of any reaction depends only on the reactant concentrations.
Hence the rate law of above reaction can be written as
Rate = K X [ClO2 ]a X [OH- ]b
K = Rate constant
where [OH- ] = concentration of OH- ions
[ClO2 ] = concentration of ClO2 ions
a = order of reaction with respect to ClO2
b = order of reaction with respect to OH-
a) Hence substituting the given values we get
1) 0.0248 = K X (0.060)a X (0.030)b
2) 0.00276 = K X (0.020)a X (0.030)b
3) 0.00828 = K X (0.020)a X (0.090)b
Dividing equation 1 from equation 2 we get
9 = 3a => a = 2
Dividing equation 3 from 2 we get
3 = 3b => b = 1
Hence the rate law for the reaction = K X [ClO2 ]2 X [OH- ]
Step by step
Solved in 3 steps
