For the reaction A + 2B → 3C + D, the rate of appearance of C, d[C]dt is equal to:

Match List I (Order of reaction) with List II (Unit of rate constant): List I: A. Zero order B. First order C. Second order D. Third order List II: I. mol-1 L s-1 II. mol-2 L2 s-1 III. s-1 IV. mol L-1 s-1 Choose the correct matching:

Given below is an expression for the rate constant of a first order reaction occurring at a certain temperature, T (K): ln k = 14.34 - 1.25 × 104T The energy of activation in kcal mol-1 for the reaction is: (Given: k in s-1, R = 1.987 cal mol-1 K-1)

For a certain reaction R → Product, the plot of concentration [R] vs time has a negative slope. The order of reaction is:

The simple collision theory of reaction rates is strictly applicable to:

The unit of rate constant for a zero-order reaction is:

The order of reaction for the inversion of cane sugar: C12H22O11 + H2O H+ C6H12O6 + C6H12O6 is:

Consider the gas phase reaction (Lindemann-Hinshelwood mechanism): A + B ⇌ A* + B (forward rate constant k1, reverse rate constant k-1) A* → C (rate constant k2) Considering [A]0 and [B]0 to be moderate and using steady state approximation, what is the overall order of the reaction?

An enzyme (E) catalyzes the conversion of a substrate (S) to product (P) according to the mechanism: E + S ⮈ ES (k1, k-1) → ES' (k2) → E + P (k3) Applying steady state approximation to ES and ES', the expression for the rate of reaction (where [E]0 and [S]0 are initial concentrations and [S]0 >> [E]0) is: