calcium oxide and water experiment

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• National Center for Biotechnology Information - PubMed Central - Accidental Ingestion of Quicklime
• Academia - Factors influencing the reactivity of quicklime

quicklime (CaO) , compound of one atom of calcium and one atom of oxygen that is a white or grayish white solid produced in large quantities by roasting calcium carbonate so as to drive off carbon dioxide . At room temperature, CaO will spontaneously absorb carbon dioxide from the atmosphere , reversing the reaction. It will also absorb water , converting itself into calcium hydroxide and releasing heat . The bubbling that accompanies the reaction is the source of its name as “quick,” or living, lime. The reaction of quicklime with water is sometimes used in portable heat sources.

One of the oldest known products of a chemical reaction , quicklime is used extensively as a building material. The origin of hydraulic cements goes back to ancient Greece and Rome. The materials used were lime and a volcanic ash that slowly reacted with it in the presence of water to form a hard mass. This served as the cementing material of the Roman mortars and concretes of more than 2,000 years ago and of subsequent construction work in western Europe.

Large quantities of quicklime are used in various industrial neutralization reactions. In steelmaking, quicklime is added to molten iron , where it reacts with impurities in the iron to form slag , which can be easily removed, thus helping to improve the purity of the steel . Calcium oxide is used with calcium hydroxide in treating water to make it safe for drinking; adding these chemicals increases the water’s alkalinity , which kills microorganisms. Limelights , used in the 19th century in stage lighting, emit a very brilliant white light upon heating a block of calcium oxide to incandescence in an oxyhydrogen flame (hence the expression “to be in the limelight”).

The most common form of glass , soda-lime glass , is composed of about 70 percent silica (silicon dioxide), 15 percent soda (sodium oxide), and 9 percent quicklime, with much smaller amounts of various other compounds . The soda serves as a flux to lower the temperature at which the silica melts, and the quicklime acts as a stabilizer for the silica. Soda-lime glass is inexpensive, chemically stable, reasonably hard, and extremely workable, because it is capable of being resoftened a number of times if necessary to finish an article.

Calcium oxide has a melting point of 2,572 °C (4,662 °F) and a boiling point of 2,850 °C (5,162 °F). It has a molecular weight of 56.08 grams per mole .

• Chemical Compound Formulas
• Calcium Oxide

Calcium Oxide - CaO

What is calcium oxide (cao) .

Calcium oxide, commonly known as lime, is a chemical compound with the formula CaO.

Calcium oxide, also known as quicklime , is an alkaline substance that has been in use since the medieval age. It is believed that quicklime is one of the oldest chemicals known to the human race. It can also be referred to as burnt lime or lime .

Table of Contents

Preparation of calcium oxide, structure of cao molecules, lime water formula, properties of calcium oxide, uses of calcium oxide, important safety tips.

• Frequently Asked Questions – FAQs

Calcium oxide has a medium viscosity and a high surface tension, plus a high to intermediate expansion and contraction rate. This material isn’t volatile at ceramic temperatures. Calcium oxide has a moderate effect on colour, except in large amounts when it may have a bleaching effect on iron oxide. It also exists in the colour of kaki/tomato reds.

• Calcium oxide can be produced by thermal decomposition of materials like limestone or seashells that contain calcium carbonate (CaCO 3 ; mineral calcite) in a lime kiln.
• The process that is used to prepare burnt lime is known as calcination. It is a process that starts with thermally decomposing the reactants at high temperatures but ensuring that the temperature is kept well below the melting point .
• Calcium carbonate undergoes calcination at temperatures ranging between 1070 o C-1270 o C. These reactions are usually held in a rotary kiln. The products formed as a result of the reaction are burnt lime and carbon dioxide.

The carbon dioxide that is formed is immediately removed so that the reaction is preceded until the completion of the process in accordance with Le-Chatelier’s principle .

CaCO 3 → CaO + CO 2

This reaction is reversible and exothermic in nature in the forward direction.

Calcium oxide molecules contain one calcium cation (which holds a charge of +2) and one oxygen anion (which holds a charge of -2). The structure of calcium oxide is illustrated below.

Thus, it can be understood that calcium oxide is an ionic compound featuring an ionic bond between calcium and oxygen.

The formula for lime water is Ca(OH) 2  and the chemical name for lime water is calcium hydroxide. When water is added to lime calcium hydroxide Ca(OH) 2 is formed according to the following reaction.

CaO + H 2 O → Ca(OH) 2

This reaction is strongly exothermic and takes place vigorously with the formation of clouds of steam.

What is the Difference Between Quicklime and Lime Water?

The chemical formula of lime or quicklime is CaO. The chemical name of lime is calcium oxide. On the other hand, the chemical formula of limewater is Ca(OH) 2 and the chemical name of this substance is calcium hydroxide.

• Quick lime is an amorphous white solid with a high melting point of 2600 °
• It is a very stable compound and withstands high temperatures.
• In the presence of water, it forms slaked lime. This process is called the slaking of lime.

CaO+H 2 O → Ca (OH) 2

• It is an oxide that is basic in nature and forms salts when it comes in contact with an acid.
• This compound crystallizes in a cubic crystal lattice.
• The standard molar entropy associated with calcium oxide corresponds to 40 joules per mole kelvin.
• This compound is known to emit an intense glow when it is heated to temperatures above 2400 degrees celsius.

CaO+H 2 SO 4 → CaSO 4 +H 2 O

• It is extensively used for medicinal purposes and insecticides.
• It finds its application in the manufacturing of cement, paper, and high-grade steel.
• Lime is used as a reagent in laboratories for dehydration, precipitation reaction , etc.
• It is the cheapest alkali available which is an important ingredient in the manufacturing of caustic soda.
• Calcium is essential to animal life as the constituent of bones, shells, and teeth. The most common of the calcium compounds are calcium carbonate which the potter uses as a source of calcium oxide for glazes.
• There are few things that users should keep in mind regarding Calcium Oxides.
• The reaction between quicklime and water is usually vigorous.
• Quicklime can cause severe irritation, especially when inhaled or if it comes in contact with wet skin or eyes.
• Some of the effects of inhalation include sneezing, coughing, or laboured breathing.
• Additionally, it can also result in abdominal pain, nausea burns with perforation of the nasal septum, and vomiting.
• When quicklime reacts with water it can release enough heat to even ignite combustible materials.

Frequently Asked Questions – FAQs

Who discovered calcium oxide.

It was first discovered in England in 1808 when a combination of lime and mercuric oxide was electrolyzed by Sir Humphry Davy.

Can you drink Limewater?

Lime water mimics hydrochloric acid which is found in the stomach and, therefore, helps prevent constipation and conditions such as diarrhoea.

Why is calcium important for bones?

Calcium makes bones more brittle. Getting enough calcium in your diet not only maintains healthy bones but also may help prevent hypertension.

What are the two uses of quicklime?

It is used as a basic flux. It is used in the refining of sugar and as a disinfectant and germicide.

Does calcium oxide dissolve in water?

Calcium oxide dissolves in water and glycerol.

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The composition and formula of water

In association with Nuffield Foundation

• No comments

Try this demonstration to determine the formula of water through the reaction of copper(II) oxide with hydrogen

In this experiment, students observe as a known mass of heated copper(II) oxide is reduced in a stream of hydrogen gas. The water formed by this reaction is then absorbed by sulfuric acid or anhydrous calcium chloride granules.

The loss in mass of the oxide is equal to the mass of the oxygen in the water, while the gain in mass of the whole apparatus is equal to the mass of the hydrogen in the water. From these results, students can work out the percentage by mass composition of water and deduce its formula.

This demonstration extends the investigation of the volumes of hydrogen and oxygen that combine (see this experiment exploring the  combustion of hydrogen in air ) to a more quantitative level involving reacting masses. It requires careful rehearsal if results approaching the expected values for the composition of water are to be obtained.

The ratio of the reacting masses can be used to deduce a relative atomic mass for oxygen, based on hydrogen. The reacting masses can also be used to deduce the formula for water and the balanced equation for its formation. This could be extended to a treatment using the mole concept with suitable groups.

The time for carrying out the demonstration should be about 30–40 minutes.

• Eye protection for demonstrator
• Safety screens
• Side-arm test tubes, 140 x 22 mm, x2
• Test tubes, x2
• One-hole bung, to fit side-arm tubes, x2
• Right-angled glass delivery tubes, x2
• Short length of glass tubing, to fit bung
• Combustion tube, about 15 cm long
• Drying tube
• One-holed bung, to fit drying tube
• Right-angled glass tube with jet
• Short lengths of rubber tubing
• Glass or ceramic wool
• Dropping pipette teats, to seal glass tubes, x2
• Bunsen burner
• Access to a balance
• Boss, clamp and stand
• Copper(II) oxide, wire form, (HARMFUL, DANGEROUS FOR THE ENVIRONMENT), 25–30 g
• Concentrated sulfuric acid (CORROSIVE), about 20 cm 3
• Anhydrous calcium chloride granules (IRRITANT), enough to fill drying tube
• Access to a supply of hydrogen (EXTREMELY FLAMMABLE), cylinder or chemical generator – see these standard techniques for generating, collecting and testing gases

Health, safety and technical notes

• Read our standard health and safety guidance.
• Wear eye protection throughout.
• Copper(II) oxide, CuO(s), purchased in wire form (HARMFUL, DANGEROUS FOR THE ENVIRONMENT) – see CLEAPSS Hazcard HC026 . The copper(II) oxide should be thoroughly dried by heating at 300–400 °C for a few minutes and stored, when cool, in a desiccator.
• Concentrated sulfuric acid (CORROSIVE) – see CLEAPSS Hazcard HC098a . 
• Anhydrous calcium chloride, CaCl 2 (s), (IRRITANT) – see CLEAPSS Hazcard HC019A . The anhydrous calcium chloride must be freshly opened or thoroughly dried by heating in a Bunsen flame and stored, when cool, in a desiccator.
• Hydrogen, H 2 (g), (EXTREMELY FLAMMABLE) – see CLEAPSS Hazcard HC048 . Using hydrogen from a gas cylinder will be much more efficient in flushing the air out of the apparatus, which has quite a considerable total volume.
• Place 25 – 30 g of dry wire-form copper(II) oxide in the combustion tube and secure in it place with tufts of glass or ceramic wool. Fit the bung and glass tube. Weigh the tube and its contents.
• Place a few cm 3 of concentrated sulfuric acid in each of the side-arm test tubes and fit the bungs carrying the delivery tubes. Make sure that the ends of the tubes are below the level of the acid. Connect one of the side-arm tubes to the exit end of combustion tube, as shown in the figure below. Seal the ends of this assembly with pipette teats and weigh it.

Source: Royal Society of Chemistry

How to set up the equipment required to determine the percentage by mass composition of water via the reduction of copper(II) oxide with hydrogen gas, using sulfuric acid and anhydrous calcium chloride to absorb the water produced

• Attach the second side-arm tube to the end of the combustion where the hydrogen gas enters, to capture any moisture in the gas. Fill the drying tube with anhydrous calcium chloride granules using a plug of glass or ceramic wool to hold them in position. Add the tube carrying the jet and join the drying tube to the rest of the apparatus, as shown in the diagram above. Seal the apparatus with the teats again.
• Clamp the apparatus in position, remove the teats and connect it to the hydrogen supply, set beforehand to deliver a steady stream of gas.
• It is most important to test the gas passing through the apparatus before heating is begun, As the apparatus has a considable volume, it will take time to flush out all the air. Take samples of the gas issuing from the jet using an inverted test tube. Attempt to ignite the hydrogen by passing the mouth of the test tube through a Bunsen flame situated at a safe distance from the apparatus. If it ignites with a pop then there is still air in the mixture. If it merely ignites and burns smoothly, this indicates that the gas is almost pure hydrogen.It should then be possible to use the burning gas to light the hydrogen jet.
• Now heat the contents of the combustion tube with a medium-sized Bunsen flame until all the copper oxide has been reduced to copper. It will change colour from black to a bright, pinkish-coloured solid. Water will condense inside the combustion tube. It is important to reduce all the oxide and to continue heating until no more moisture comes out of the combustion tube and is absorbed by the sulphuric acid or the drying tube.
• Continue the flow of gas until the combustion tube has cooled down. Stop the gas flow and disconnect it from the apparatus. Remove the first side-arm tube and the drying tube and seal the combustion tube + second side-arm tube assembly using the two teats. Weigh it as a whole before removing the combustion tube and weighing it separately.

Teaching notes

The redox reaction is simply: CuO(s) + H 2 (g) → Cu(s) + H 2 O(l)

Use the masses of the combustion tube before and after heating to work out the mass of oxygen lost by the copper(II) oxide and now present in the water formed.

Use the mass of the whole apparatus before and after heating to work out the mass of water formed and hence the mass of hydrogen in it by subtracting the mass of oxygen. As the oxygen is only transferred from the copper oxide to form water inside the apparatus, any gain in mass is due to hydrogen combined with the oxygen to form water.

The ratio of the two masses enables the mass of oxygen combining with 1 g of hydrogen to be calculated. It should be close to 8 g if all has gone well. Point out that this would give oxygen a relative mass of 8 on a scale where H = 1, if the formula of water was HO. 

However, as the relative mass of an oxygen atom is 16, this mass ratio is in accordance with a formula for water of H 2 O.

Additional information

This is a resource from the  Practical Chemistry project , developed by the Nuffield Foundation and the Royal Society of Chemistry.

Practical Chemistry activities accompany  Practical Physics  and  Practical Biology .

© Nuffield Foundation and the Royal Society of Chemistry

• 14-16 years
• 16-18 years
• Demonstrations
• Redox chemistry
• Quantitative chemistry and stoichiometry
• Equations, formulas and nomenclature

Specification

• 8. be able to calculate reacting masses from chemical equations, and vice versa, using the concepts of amount of substance and molar mass
• Students should be able to use balanced equations to calculate: masses.
• e) calculations, using amount of substance in mol, involving: mass, gas volume, solution volume and concentration
• Calculate the masses of reactants and products from the balanced symbol equation and the mass of a given reactant or product.
• Use a balanced equation to calculate masses of reactants or products.
• 1.48 Calculate masses of reactants and products from balanced equations, given the mass of one substance
• C5.3.7 use a balanced equation to calculate masses of reactants or products
• C5.2.7 use a balanced equation to calculate masses of reactants or products
• C1.3n use a balanced equation to calculate masses of reactants or products
• C1.3l use a balanced equation to calculate masses of reactants or products
• (d) how empirical and molecular formulae can be determined from given data
• (p) how to calculate the formula of a compound from reacting mass data
• 1.7.5 calculate the reacting masses of reactants or products, given a balanced symbol equation and using moles and simple ratio, including examples here there is a limiting reactant;
• 1.7.7 recognise possible reasons why the percentage yield of a product is less than 100%, including loss of product in separation from the reaction mixture, as a result of side reactions or because the reaction is reversible and may not go to completion;
• 1.7.6 calculate the reacting masses of reactants or products, given a balanced symbol equation and using moles and simple ratio, including examples here there is a limiting reactant;
• 1.7.8 recognise possible reasons why the percentage yield of a product is less than 100%, including loss of product in separation from the reaction mixture, as a result of side reactions or because the reaction is reversible and may not go to completion;

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Synthesis and Application of Ti/La Based Composite Catalyst for Triglyceride Conversion into Biodiesel

• Original Paper
• Published: 20 August 2024

Cite this article

• Hamza Zahoor 1 ,
• Romana Khan   ORCID: orcid.org/0000-0003-2760-0914 2 ,
• Sadia Nasreen 3 ,
• Syed Nasir Shah 4 ,
• Raja Muhammad Asif Khan 5 ,
• Muhammad Usman 6 &
• Ihsanullah Sohoo 7  

The search for substitute fuels has motivated researchers to explore alternate attractive options such as conversion of used oils to biodiesel. This study is focused on the production of biodiesel from waste cooking oil by developing a porcelain supported titanium and lanthanum oxide based composite catalyst. This heterogeneous composite catalyst was synthesized by the wet-impregnation method. The reaction procedure as well as reaction parameters like methanol to oil molar ratio, different catalyst loading, reaction temperature, reaction time, and reusability of catalyst was investigated. The results show that with the help of Ti: La: Porcelain, the yield of biodiesel produced was 94% at ≥ 90 ° C in 7 h. For both catalysts, 5 wt% of catalyst based on oil, 36:1 methanol/oil molar ratio was reused 5 times with regeneration. Different characterization of porcelain supported titanium and lanthanum Oxides before and after trans-esterification were performed using x-ray diffraction (XRD), scanning electron microscopy (SEM), and energy-dispersive x-ray spectroscopy (EDS) techniques. The high-performance liquid chromatography (HPLC) technique was used to analyze synthesized biodiesel. The physiochemical properties of the synthesized biodiesel were performed as well, and color changes were also scrutinized. A static immersion test of copper, aluminum, zinc, iron and stainless steel in the blend of prepared biodiesel/diesel was conducted at room temperature (25 –27 °C) for 720 h utilizing the conventional method of measuring weight loss. The findings of the study revealed that blend of biodiesel/diesel sample was less corrosive to these materials compared to literature at room temperature.

Biodiesel synthesis from low grade waste cooking oil was studied.

Developed a heterogeneous composite catalyst titanium and lanthanum oxide.

Supported catalyst on porcelain support for recovery and recycling.

Catalyst characterization using SEM, EDX, X-ray diffraction, BET surface area and Hammett indicators.

The results show using Ti: La: Porcelain catalyst the biodiesel produced was 94% at ≥ 90 ° C in 7 h under optimum conditions.

The blend of biodiesel/diesel produced was of good quality and less corrosive compared to literature at room temperature.

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Data Availability

The datasets generated during and/or analyzed during the current study are available from the corresponding author on reasonable request.

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Authors are grateful to the Department of Environmental Engineering, University of Engineering and Technology Taxila for providing the materials, equipment and space used in this study.

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Romana Khan

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Sadia Nasreen

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Zahoor, H., Khan, R., Nasreen, S. et al. Synthesis and Application of Ti/La Based Composite Catalyst for Triglyceride Conversion into Biodiesel. Waste Biomass Valor (2024). https://doi.org/10.1007/s12649-024-02689-9

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