Hydrogen iodide decomposes according to the equation 2HI(g)   ↔   H2(g) + I2(g), for which Kc = 0.0156  at 400ºC.  0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium.

For the following reaction at equilibrium, which one of the changes below would cause the equilibrium to shift to the left? 2NOBr(g)   ↔   2NO(g) + Br2(g),     DHºrxn = 30 kJ/mol

Choose the response that lists the member of each of the following pairs that has the higher boiling point. (I) H2O or KI       (II) HF or HI      (III) Cl2 or Br2

0.204 g of an unknown compound dissolved in 180 mL of water has an osmotic pressure of 26.2 mmHg at 24.0°C.  Calculate the molar mass of the compound. (R = 0.0821 L·atm/K·mol)

For the reversible reaction SO2(g) + NO2(g)   ↔   SO3(g) + NO(g), the equilibrium constant is 18.0 at 1,200ºC.  If 1.0 mole of SO2 and 2.0 moles of NO2 are placed in a 20 L container, what concentration of SO3 will be present at equilibrium?

A 0.10 M NH3 solution is 1.3% ionized.  Calculate the H+ ion concentration.             NH3 + H2O → NH4+ + OH–

What is the osmotic pressure of a solution that contains 16.2 g of propyl alcohol (C3H7OH) dissolved in enough water to make 400 mL of solution at 27°C?

What is the molality of a solution that is 6.72 % by mass calcium chloride?

Calculate the standard enthalpy change for the reaction    2C8H18(l) + 17O2(g) ->16CO(g) + 18H2O(l).             Given: 2C8H18(l) + 25O2(g) -> 16CO2(g) + 18H2O(l)    Δ{“version”:”1.1″,”math”:”Δ”}H° = –11,020 kJ/mol 2CO(g) + O2(g) -> 2CO2(g)                              Δ{“version”:”1.1″,”math”:”Δ”}H° =   –566.0 kJ/mol

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