Problem 81 - Chemistry An Atoms First Approach

Question

Novelty devices for predicting rain contain cobalt(II) chloride and are based on the following equilibrium:$$\mathrm{CoCl}_{2}(s)+6 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CoCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}(s)$$ Purple Pink.What color will such an indicator be if rain is imminent?

Step-by-Step Solution

Answer

The indicator will be Pink if rain is imminent, due to the equilibrium shift favoring the formation of cobalt(II) chloride hexahydrate (CoCl₂·6H₂O) in response to increased water vapor concentration.

Step 1: Write the balanced equation

Identify the balanced chemical equation.

Step 2: Write the equilibrium expression

Express K using product/reactant concentrations.

Step 3: Substitute and calculate

Plug in given values.

Step 4: State the result

The answer is: The indicator will be Pink if rain is imminent, due to the equilibrium shift favoring the formation of cobalt(II) chloride hexahydrate (CoCl₂·6H₂O) in response to increased water vapor concentration.

Key Concepts

Chemical Equilibrium

Understanding the dynamics of chemical reactions is fundamental to the study of chemistry, and chemical equilibrium plays a key role in this. At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction, meaning the reactants and products are formed at the same rate. In our exercise, we have the equilibrium between anhydrous cobalt(II) chloride and its hydrated form, cobalt(II) chloride hexahydrate.

The reaction can be represented as: \[\text{CoCl}_2(s) + 6\text{H}_2\text{O}(g) \rightleftharpoons \text{CoCl}_2 \cdot 6\text{H}_2\text{O}(s)\]. In the presence of moisture (like high humidity before rain), the reaction shifts to the right, forming more of the pink hydrate. Conversely, in dry conditions, the equilibrium shifts to the left, and the anhydrous form, which has a purple color, predominates. Through Le Chatelier's Principle, we understand that a change in conditions leads to an equilibrium shift to counteract that change. This shift is what causes the color change in our hygroscopic weather predictor.

Hygroscopic Substances

Hygroscopic substances have a knack for attracting and holding water molecules from the surrounding environment through absorption or adsorption. Cobalt(II) chloride is a particularly well-known hygroscopic material that undergoes a noticeable physical change upon water absorption.

The reaction, \[\text{CoCl}_2(s) + 6\text{H}_2\text{O}(g) \rightleftharpoons \text{CoCl}_2 \cdot 6\text{H}_2\text{O}(s)\], showcases cobalt(II) chloride's hygroscopic nature as it bonds with water to form its hydrate. This property is leveraged in applications such as moisture indicators in novelty devices, desiccants for keeping goods dry, and even in laboratories to control humidity levels. Their ability to react with water vapor and change color based on the degree of hydration or dehydration makes them invaluable tools.

Predicting Weather Changes

While modern meteorology uses complex instruments and computer models to predict the weather, simple chemical principles can still provide clues about upcoming changes. Substances like cobalt(II) chloride serve as rudimentary weather prediction tools. The color change from purple to pink in the presence of moisture is a visual cue of increased humidity, which often precedes rain.

Novelty weather-indicating devices capitalize on this chemistry to provide a handy, albeit basic, forecast tool. As moisture in the air increases, these devices, containing cobalt(II) chloride, absorb water and transition to a pink state. Such rudimentary methods can be surprisingly accurate in the short term and provide a fun way to engage with the principles of science and nature.