IB DP Chemistry: HL复习笔记7.1.3 Equilibrium Constant Relationships
Equilibrium Constant Relationships
In the previous section we saw that the concentrations of the substances are raised to the?power of the coefficients?from the balanced equation
This means the?Kc?expression?is dependent on a specific equation
For example, take the reaction between nitrogen and hydrogen to make ammonia
?N2(g)??? +??? 1?H2(g)? ?? ? ?NH3(g)
The?Kc?expression for this reaction is:
If you double the stoichiometry the equation becomes
N2(g)??? +??? 3H2(g)? ? 2NH3(g)
The new?Kc?expression for this reaction is then:
What is the relationship between these two?Kc?values? You can probably see that when we double the coefficient the new?Kc is the square of the original value:
If we reverse the equation:
2NH3(g)?? N2(g)??? +??? 3H2(g)
Kc? becomes the reciprocal of the original Kc?value:
Test your understanding in the following example:
Worked Example
Kc?for 2NO2?(g) + F2?(g) ? 2NO2F (g) is 7.1 × 1032What is?Kc?for the following reaction, at the same temperature?
NO2F (g) ?? NO2?(g) + ?F2 (g)
Answer:
The correct option is?B.
The original equation has been reversed and halved, so the?Kc?value must be square rooted and inverted to obtain the reciprocal
Exam Tip
You must use square brackets in equilibrium constant expressions as they have a specific meaning, representing concentrations. In an exam answer you would lose the mark if you used round brackets
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