402Examples

# 402Examples - Lesson 17 2 Lesson 17 Example 3 A sample of...

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Lesson 17 1 Lesson 17 Example 1 The equilibrium constants for the following reactions have been measured at 823 K: CoO ( s ) + H 2 ( g ) = Co ( s ) + H 2 O ( g ) K p 1 = 67 CoO ( s ) + CO ( g ) = Co ( s ) + CO 2 ( g ) K p 2 = 490 From these data, calculate the equilibrium constant of the following reaction at 823 K: CO 2 ( g ) + H 2 ( g ) = CO ( g ) + H 2 O ( g ) Lesson 17 Chemical equilibrium calculations Lesson 17 Example 2 A mixture that was initially at 0.005 M in H 2 ( g ) and 0.0125 M in I 2 ( g ) and contained no HI ( g ) was heated at 425.4 o C until equilibrium was reached. The equilibrium concentration of I 2 ( g ) was found by experiment to be 0.00772 M. What is the numerical value of K c for the following reversible reaction? H 2 ( g ) + I 2 ( g ) = 2 HI ( g )

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Unformatted text preview: Lesson 17 2 Lesson 17 Example 3 A sample of COCl 2 is allowed to decompose. The value of K c for the reversible reaction COCl 2 ( g ) = CO ( g ) + Cl 2 ( g ) is 2.2x10 10 mol/L at 100 o C. If the initial concentration of COCl 2 is 0.095 M, what will be the equilibrium concentrations of COCl 2 , CO and Cl 2 ? Lesson 17 Example 4 For the reaction 2 CaSO 4 ( s ) = 2 CaO ( s ) + 2 SO 2 ( g ) + O 2 ( g ) at 1625 K, starting only with CaSO 4 ( s ), the total pressure at equilibrium is 0.04608 atm. What is the value of K c written with concentrations in mol/L? Lesson 17 Suggested readings 15.7 Equilibrium Calculations: Some Illustrative Examples...
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## This note was uploaded on 11/29/2011 for the course CHE 102 taught by Professor Simon during the Fall '08 term at Waterloo.

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402Examples - Lesson 17 2 Lesson 17 Example 3 A sample of...

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