Calculating K H 2 (g) + F 2 (g)  2HF(g) The equilibrium constant for the reaction above is 115 at a certain temperature. In a particular experiment, 3.00.

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Calculating K H 2 (g) + F 2 (g)  2HF(g) The equilibrium constant for the reaction above is 115 at a certain temperature. In a particular experiment, 3.00 mol of each component was added to a 1.5 L flask. Calculate the equilibrium concentration for all species.

Problem 27, p 615 At 327 o C, the equilibrium concentrations are [CH 3 OH] = 0.15 M, [CO] = 0.24 M and [H 2 ] = 1.1 M for the reaction: CH 3 OH (g)  CO (g) + 2H 2 (g) Calculate K p at this temperature.

Problem 31, p. 615 Consider the following rxn. at a certain temperature: Fe (s) + 3 O 2 (g)  2 Fe 2 O 3 (s) An equil. mixture contains 1.0 mole Fe, mole O 2 and 2.0 mole Fe 2 O 3 all in a 2.0 L container. Calculate K c for this reaction.

Problem 39, p. 616 A 1.00 L flask was filled with 2.00 mole gaseous SO 2 and 2.00 mole of NO 2 and heated After equil. was reached, it was found that 1.30 mole gaseous NO was present. Calculate the value of K c for: SO 2 (g) + NO 2 (g)  SO 3 (g) + NO (g)

Problem 52, p. 617 At a particular temperature, K c = 4.0 x for the reaction: N 2 O 4 (g)  2NO 2 (g) In an expt. 1.0 mole of N 2 O 4 is placed in a L vessel. Calculate the concentrations of N 2 O 4 and NO 2 when this reaction reaches equilibrium.

Use of Approximation Approximations can be used if the value of K is so small that the terms (-x) or (+x) will barely have an effect. Validity of approximation: < 5% ______[x]______ =< 5% [initial concentration]