8. If, for the reaction aX + bY → products, the rate law is determined to be r = k[X]'[Y]², then the overall order of reaction is а. 1 d. 4 b. 2 e. С. 3 f.
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- Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A +B −−→ P and the reactants are initially present in (a) their stoichiometric proportions, (b) with Bpresent initially in twice the amount.Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A + B → P and the reactants are initially present in (a) their stoichiometric proportions ([B]0 = 12[A]0); (b) with B present initially in twice that amount ([B]0 = [A]0). Express your rate law in terms of [A]0, [B]0, and x, where [A] = [A]0 − 2x.The rate law for a reaction was reported as v= k,[A][B][C] with the molar concentrations in moles per cubic decimetre and the time in seconds. What are the units of k,?
- a. Express the rate in terms of change of concentration of A with respect to time where 2A + B -> products, rate = k[A]-1. b. Give the derived integrated rate law.Assuming the rate law for the system is rate = k[I-]x[S2O82-]y, what is the value of x for the system? Explain your answer. What are the steps in obtaining this answer?Write down the kinetic equation for a simple reaction in a homogeneous medium 2A + B = 2C. Indicate the general and in relati on to all reactants reaction orders
- Why did the 1st order integrated rate law allow you to find k from the slope?If the rate law for the reaction bewteen NO and O2 is Rate = k[NO]3[O2] the units of k are M-1s-1 Is this true or false?Calculate the ratio of rates of catalyzed to non-catalyzed reactions at 37°C, given that the Gibbs energy of activation for a particular reaction is reduced from 100 kJ/mol to 10 kJ/mol. Ans: 1.5 x 1015
- If the rate law for a process is rate=k[A]^2 [B], and [A]=0.7085 and [B]=0.1211, determine the rate as a multiple of k. State the answer without including k.Consider the following reaction: A + B --> products. The rate law was found to be rate = k[A][B]^2. What is the order with respect to A?The rate equation for the reaction A→B + C is expressed in the forms of rate of disappearance of A = k[A]x. The value of the rate constant is 0.100(units unspecified) and [A]= 0.050 mol/L. What are the units of k and the rate reactions in mol/L-s if the reaction is second order?