In this lesson, we will learn how to construct and calculate the equilibrium constant for concentration.

Students will be able to

Q1:

Ammonia can be produced by the reaction between hydrogen and nitrogen gas that is represented by the following equation: 3H+N2NH223

5.00 mol of nitrogen gas and 5.00 mol of hydrogen gas are placed in a sealed vessel that has a volume of 20.00 dm^{3} at 500 K. At equilibrium, only 0.25 mol of nitrogen would be converted into ammonia.

Calculate the value of 𝐾 at this temperature, giving the answer to 3 decimal places.

Q2:

At equilibrium, 𝐾=32⋅moldm at 325 K for the following reaction involving oxides of sulfur: 2SO()+O()2SO()223ggg

Find the value of 𝐾, including units, at 325 K for the following reaction:

2SO()2SO()+O()322ggg

Q3:

The example equation 𝐾=[][][][]ABCD

shows how different chemical species, such as A, B, C, and D, are often enclosed in square brackets in equilibrium constant calculations.

What do the square brackets indicate?

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