a second-order reaction of the type A+2B-->P was carried out in a solution that was intially 0,050 mol dm^-3 ln A and 0,030 mol dm ^-3 ln B after 1.0 h the concentration of A had fallen to 0,010 mol dm^-3 a.  Calculate the rate constant b. What is the half-life of the reactants

The following irreversible reaction takes place in a batch reactor? → B Determine how long it takes for the conversion to reach 50%, if the reaction is a second order reaction with respect to A and kCA0 = 0.2 min-1,

Problem IX (10 p): Consider the isomerization of compound A from its cis to its trans isomer at 298 K, which is first order in both directions: ki cis-A = trans-A k2 The rate constant for the forward reaction is k1 = 4.2 × 10* s', and the rate constant for the reverse reaction is k2 = 2.1 × 10-ª s-1. %3D a) Calculate the equilibrium concentrations [cis-A]eq and [trans-A]eq, assuming that at time t= 0 all of A was in the cis-form, i.e., [cis-A]o = [A]o. (Hint: Use the fact that at any time, [cis-A] + [trans-A] = [A]o.) %3D b) Which reaction is spontaneous, the forward reaction or the reverse reaction? Provide your reasoning. Total /100 p

What is the rate for the second order reaction A Products when [A] = 0.207 M? (k = 0.761 M 's )

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