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The equilibrium constant is given for one of the reactions below.  Determine the value of the missing equilibrium constant. N2O4 (g) ⇌ 2NO2 (g)                 Kc = 1.46                                                      6NO2 (g) ⇌ 3 N2O4 (g)       Kc  = ?

Identify the change in state whereΔS decreases.

Of the following. which acids are weak acids? I. HBr II. HF III. HNO3 IV. HNO2 V. H2CO3 VI. H3AsO4

Use the standard half-cell potentials listed below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25 OC. 3Cl2 (g) + 2Fe (s) à 6 Cl- (aq) + 2 Fe3+ (aq)             Cl2 (g) + 2 e- à 2Cl- (aq)                   EO = +1.36 V             Fe3+ (aq) + 3 e- à Fe (s)                  EO = -0.04 V

According to Lewis theory, a base……

A reaction is shown below                     2A + 3B →  Products   Experiment     Initial [A]     Initial [B]    Initial Rate (M.s -1)            1     0.10 M     0.30 M       7.20 X 10 -5            2     0.10 M     0.60 M       1.44 X 10 -4 What is the reaction order for reactant B?  Hint: rate of reaction = K [A]m X [B]n ; K is a constant

What is the Kb of a weak base if a 0.250 M solution has a pH of 11.59?

Which of the following compound is incorrectly identified as to type of compound it is?          Substance        Type of compound    A KOH Strong base B HClO 4 Strong acid C HNO 2 Weak acid D NH 3 Insoluble base (in water) E H 2SO 3 Weak acid

From a consideration of the Lewis structure (see the attached file below), what are the formal charges? Question 68.docx        N   C   O   (A)  -1   0   0  (B)  -1  +1   -1  (C)  0  0  0  (D)   0  0   -1  (E)   -2  0   +1

The rate constant for the first-order decomposition of N2O is 3.40 s-1. What is the half-life of the decomposition? ** Don’t forget the units. round to the third decimal place [BLANK-1]