The reaction between calcium carbonate and hydrochloric acid

THE REACTION BETWEEN CALCIUM CARBONATE AND HYDROCHLORIC ACID 

In this reaction we could monitor how fast carbon dioxide gas or calcium chloride was being made, or how quickly calcium carbonate or hydrochloric acid was being used up. The simplest method is to track the amount of carbon dioxide evolved, which can be done in two ways. 

Both graphs show the progress of the same reaction 

The rate of the reaction, at a specific time, can be worked out by finding the slope or gradient of a tangent to the curve at that time. 

To quote the rate of the reaction in terms of how many moles per second of carbon dioxide are being formed it is necessary to use the stoichiometric equation and scale the quantities accordingly  

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Alternatively, a reaction producing a gas can be performed in an open flask placed on an electronic balance. The reaction can then be investigated by recording the loss of mass as the gas is produced. This is shown in Figure 6.33 for the reaction between calcium carbonate and hydrochloric acid. Figure 6.34 shows the effect of chip size on a graph of mass of flask and contents versus time. 

Figure 1.13 The reaction between calcium carbonate and hydrochloric acid. The equation for this reaction, with all the state symbols, is ...

The reaction can be monitored by measuring the change in volume of gas released with time. You may have used this method to follow the rate of the reaction between calcium carbonate and hydrochloric acid. If you did, you will have measured the change in volume of carbon dioxide gas released with time. 

Figure 5.2.3 shows the results of these methods and how the rate of a reaction between calcium carbonate and hydrochloric acid varies with time. The graphs have different shapes because one charts the change in formation of carbon dioxide, i.e. the products, and the other shows how the reaction changes with relation to the reactants, i.e. how fast the system loses mass as the calcium carbonate and hydrochloric acid react to form carbon dioxide. 

Figure 6.31 shows apparatus suitable for investigating the reaction between calcium carbonate and dilute hydrochloric acid. This arrangement ensures the two reactants are kept separate while the apparatus is set up so that the start time can be accurately recorded. 

The reaction between calcium carbonate and dilute hydrochloric acid... 

Consider again the reaction between calcium carbonate, as marble chips, and hydrochloric acid. 

Increasing the surface area of a solid-phase reactant in a reaction between a solid and a liquid will enhance the rate of reaction. This is because the reaction takes place at the boundary between the two phases, that is, on the sohd surface. Commonly, the effect of increasing surface area in the reaction between calcium carbonate (marble chips) and hydrochloric acid (see equation, page 149) is used as an investigation. Other reactions also illustrate the same point. 

Table 11.11 and Figure 11.23 summarize some idealized experimental data from the reaction between excess powdered calcium carbonate and hydrochloric acid. 

Calcium carbonate is insoluble in water. Yef it dissolves in an acidic solution. Calculate the standard enthalpy, entropy, and Gibbs free energy change for the reaction between sohd calcium carbonate and hydrochloric acid. What drives the reaction, the enthalpy change, or the entropy change ... 

Properties On ignition, reaction between zinc dust and hexachlorethane produces zinc chloride and free carbon, both of which pass off in the smoke. The ammonium perchlorate keeps the reaction going, ammonium chloride readily volatilizes and controls the rate of burning, and calcium carbonate stabilizes the mixture by taking up any hydrochloric acid which may be present. The smoke is harmless. 

Table 5.1.1 Table of results obtained in the study of the reaction between dilute hydrochloric acid and calcium carbonate, as large marble chips... 

The enthalpies of reactions between alkaline-earth cuprates M2CUO3 (M = Ca, Sr) and hydrochloric acid were measured in a hermetic swinging calorimeter at 298.15 K. The M2CUO3 samples were prepared by solid-phase synthesis from calcium or strontium carbonate and copper oxide. The standard enthalpies of formation obtained for the cuprates were discussed and compared with previous experimental and assessed values by Monayenkova and coworkers [102]. 

Many chemical reactions go to completion. This means that the reaction continues until all component particles (whether ions, molecules or atoms) of one reagent have reacted, then stops. The reaction between hydrochloric acid and marble chips (calcium carbonate) is an example ... 

About half of the hydrochloric acid produced annually in the United States (3.0 biUion pounds) is used for metal pickling. This process involves the removal of metal oxide layers from metal surfaces to prepare them for coating, (a) Write the overall and net ionic equations for the reaction between iron(lll) oxide, which represents the rust layer over iron, and HCl. Identify the Bronsted acid and base, (b) Hydrochloric acid is also used to remove scale (which is mostly CaC03) from water pipes. Hydrochloric acid reacts with calcium carbonate in two stages the first stage forms the bicarbonate ion, which then reacts further to form carbon dioxide. Write equations for these two stages and for the overall reaction. 

In many reactions, one of the reactants is a solid. The reaction between hydrochloric acid and calcium carbonate (marble chips) is one example. Carbon dioxide gas is produced ... 

Toilet bowl cleaners often contain hydrochloric acid, which dissolves the calcium carbonate deposits that accumulate within a toilet bowl. What mass of calcium carbonate (in grams) can 3.8 g of HCl dissolve (Hint Begin by writing a balanced equation for the reaction between hydrochloric acid and calcium carbonate.)... 

Carbon dioxide is present in air and is a constituent of natural gas escaping from mineral springs and fissures in the earth s surface. It is also the ultimate product of combustion of carbon and its compounds. Laboratory scale preparation usually entails reaction between dilute hydrochloric acid and marble (calcium carbonate) ... 

A 6.53-g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces 1.72 L of carbon dioxide gas at 28 °C and 743 torr pressure, (a) Write balanced chemical equations for the reactions that occur between hydrochloric acid and each component of the mixture, (b) Calculate the total number of moles of carbon dioxide that forms fiom these reactions, (c) Assuming that the reactions are complete, calculate the percentage by mass of magnesium carbonate in the mixture. 

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