2 HI H2 + I 2
Keq = 2.06 x 10-2 @ 458°C
If both hydrogen and iodine are measured to have concentrations of 0.0135 M each at 458°C, what is the concentration hydrogen iodide?
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Fall 2005 |
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| Exercise: Chemical Equilibrium |
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Example 1: Consider the gas phase reaction:
2 HI
Keq = 2.06 x 10-2 @ 458°C
If both hydrogen and iodine are measured to have concentrations of 0.0135 M each at 458°C, what is the concentration hydrogen iodide?
Example 2: Consider the gas phase reaction:
2 HBr
Keq = 1.5 x 10-5 @ 1400 K Calculate the concentrations of all species at equilibrium if we start with 0.15 moles each of hydrogen bromide and bromine in a 0.500 L container at 1400 K.
Example 3: Consider the gas phase dissociation of carbon dioxide to carbon monoxide and oxygen @ 1000 K.
If 0.200 moles of carbon dioxide is placed in a 1.00 L container at 1000 K calculate the concentrations of all species at equilibrium. Keq = 4.5 x 10-23 @ 1000 K.
Example 4: What is the concentration of hydrogen ion in a 0.20 M solution of acetic acid (CH3COOH) if Ka = 1.8 x 10-5 @ 25°C? ( Ka is the equilibrium constant for an acid dissociation.)
Example 5: Calculate the solubility of calcium carbonate. CaCO3 is used by organisms to make shells etc. Vast deposits of these shells make up limestone and (after heat and compression) marble deposits. An important consideration in determining whether shells can be formed, limestone deposited etc. is the solubility of calcium carbonate. Ksp = 8.7 x 10-9
Example 6: Calculate the the Ksp for lead(II) chloride at 25°C if its solubility = 1.62 x 10-2 M.
Example 7: What is the solubility of ferric hydroxide in a buffered aqueous solution where [OH-] = 1 x 10-6M. Ksp = 4 x 10-38
© R A Paselk
Last modified 23 June 2006