1. The value of ΔHo for the reaction below is -228 kJ. Calculate
the value of ΔHorxn (in kJ) when 2.59 moles of NaOH (s) is formed
in the reaction?
2 Na2O2 (s) + 2 H2O (l) → 4 NaOH (s) + O2 (g)
2.The value of ΔHo for the reaction below is -721 kJ.
2 S (s) + 3 O2 (g) → 2 SO3 (s)
amount of heat released during the reaction of 6.64 grams of S
. The reaction of 2O3(g) → 3O2(g) has the experimental rate:
rate = k[O3]2 [O2]—1. The following mechanism has been proposed: 1.
O3 O2 + O fast, equilibrium 2. O + O3 → 2 O2 slow (A) Identify any
intermediates. (B) What is the rate law predicted by this
mechanism? (C) Is the rate law predicted by the mechanism
consistent with the experimental rate law? (D) How would adding a
catalyst effect this reaction?
1. KClO3 decomposes according to the
2KClO3 → 2KCl + 3O2
If the rate of decomposition of
potassium chlorate at a certain time is determined to be 2.4 x
s-1, what is the
rate of formation of KCl at the same time?
2. The rate law for a reaction involving only A and B is
1st order in A and 4th order in B,
respectively. If the concentration of A is increased by a factor of
Calculate the enthalpy of the reaction
given the following pertinent information:
Express your answer with the appropriate units.