Given the equation below, how does the rate of disappearance of O2 compare to the rate of disappearance of C3H8?C3H8 + 5 O2 → 3 CO2 + 4 H2OQuestion 2Select one:a.O2 gets used up five times faster than C3H8.b.O2 gets used up one third as fast as C3H8.c.O2 gets used up three times faster than C3H8.d.O2 gets used up one fifth as fast as C3H8.

The reaction 2NO2 → 2O2 + N2 is a third order reaction with respect to NO2. If the rate of disappearance of NO2 is 25.0 mol/Ls when the concentration of NO2 is 0.10 mol/L, what is the new rate when the concentration of NO2 changes to 0.30mol/L.

Decomposition of H2O2 follows a first order reaction. In fifty minutes the concentration of H2O2 decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H2O2 reaches 0.05 M, the rate of formation of O2 will be:

Suppose the decomposition of ozone proceeds by the following mechanism:step elementary reaction rate constant1 O3(g) → O2(g) + O(g) k12 O3(g) + O(g) → 2O2(g) k2Suppose also k1≫k2. That is, the first step is much faster than the second.Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. =ratek Note: your answer should not contain the concentrations of any intermediates.Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. =k

Which of the following would effuse at a rate equal to 31.5% of the rate of H2?COHCNCOCl2NeNH3

Consider two reactions, one that is second order and one that is third order. Which best describes the effect on the reaction rates by DECREASING the concentration of all reactants?Select answer from the options below