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What is the conjugate acid of HCO3-?

Determine the solubility of N2 in water exposed to air at 25 °C is the atmospheric pressure is 1.2 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry’s law constant for nitrogen in water at this temperature is 6.1 X 10-4 M/atm.

The overall order of the following reaction is ______.   (**Just give the whole number i.e. 1 for 1st, 2 for 2nd, 3 for 3rd ect….) 2X + 3Y à 2Z                               Rate = k[BLANK-1][BLANK-2]2

Balance the following redox reaction if it occurs in an acidic solution. What are the coefficients in front of H2C2O4 and H2O in the balanced reaction? MnO4- (aq) + H2C2O4 (aq) à Mn2+ (aq) + CO2 (g)

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