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The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 × 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K. Determine the activation energy for this reaction.

Calculate ΔS°rxn for the following reaction. The S° for each species is shown below the reaction.                        N2H4(l) + H2(g) → 2 NH3(g)  S° (J/mol∙K)  121.2       130.7         192.8

Identify the rate-determining step.

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO3(g). 2 SO2(g) + O2(g) ⇌ 2 SO3(g)   Kc = 1.7 × 108 [SO2]eq = 0.0034 M                           [O2]eq = 0.0018 M

A reaction occurs via the following sequence of elementary steps. What is the rate law based on this reaction mechanism? 1st step: A ⇌ B              very fast 2nd step: B + C → D     slow 3rd step: D → 2E          fast

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.5 M, [H2]eq = 1.1 M, [NH3]eq = 0.47 M. N2(g) + 3 H2(g) ⇌ 2 NH3(g)

Consider a reaction that has a positive ΔH and a negative ΔS. Which of the following statements is TRUE?

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(l)       ΔH° = -2220 kJ

Write a balanced reaction for which the following rate relationships are TRUE.             Rate =  =  = –  

The rate constant for the first-order decomposition of N2O is 3.40 s-1. What is the half-life of the decomposition?