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Chapter 5: Problem 120

Write an equation to show how sulfuric acids in acid rain reacts with marble and limestone. (Both marble and limestone are primarily calcium carbonate.)

Short Answer

Expert verified
The balanced chemical equation for the reaction between sulfuric acid (found in acid rain) and calcium carbonate (found in marble and limestone) is: \( H_2SO_4 + CaCO_3 \rightarrow H_2O + CO_2 + CaSO_4 \) This reaction produces water (H鈧侽), carbon dioxide (CO鈧�), and calcium sulfate (CaSO鈧�).

Step by step solution

01

Identify the reactants

The reactants in this reaction are sulfuric acid (H鈧係O鈧�) and calcium carbonate (CaCO鈧�). Sulfuric acid is the major component of acid rain, and calcium carbonate is the primary compound found in marble and limestone.
02

Predict the products

Due to the reaction between sulfuric acid and calcium carbonate, water (H鈧侽), carbon dioxide (CO鈧�), and calcium sulfate (CaSO鈧�) are formed as products.
03

Write the unbalanced equation

Now we can write the unbalanced chemical equation: H鈧係O鈧� + CaCO鈧� 鈫� H鈧侽 + CO鈧� + CaSO鈧�
04

Balance the equation

To balance this chemical equation, we can observe that the number of atoms of each element is conserved on both sides of the equation. As the given unbalanced equation already has an equal number of atoms for each element on both sides, it is balanced as follows: H鈧係O鈧� + CaCO鈧� 鈫� H鈧侽 + CO鈧� + CaSO鈧� Now the equation is balanced and represents the reaction between sulfuric acid in acid rain and calcium carbonate in marble and limestone.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Sulfuric Acid
Sulfuric acid, with the chemical formula \(H_2SO_4\), is a highly corrosive mineral acid. It plays a significant role in various chemical reactions due to its strong acidic properties. In the environment, it becomes a primary component of acid rain. This occurs when sulfur dioxide \(SO_2\) released from burning fossil fuels combines with water in the atmosphere. The result is a dilute sulfuric acid that can have damaging effects on buildings and statues made of materials like marble and limestone.
  • Sulfuric acid is colorless and viscous, often recognized for its dehydrating and oxidizing properties.
  • Its presence in acid rain contributes to the corrosion of certain minerals, including the calcium carbonates found in marble and limestone.
  • The interaction between sulfuric acid and materials like marble leads to chemical reactions that can weaken stone structures.
Understanding sulfuric acid鈥檚 role in environmental chemistry helps in mitigating its harmful effects.
Calcium Carbonate
Calcium carbonate \(CaCO_3\) is a common substance found in rocks as the minerals calcite and aragonite. Marble and limestone are primarily composed of calcium carbonate. These rocks are often used in architecture and art due to their aesthetic properties. When sulfuric acid from acid rain interacts with calcium carbonate, a chemical reaction occurs, leading to the formation of new substances.
  • The reaction between calcium carbonate and sulfuric acid produces calcium sulfate \(CaSO_4\), carbon dioxide \(CO_2\), and water \(H_2O\).
  • This process is responsible for the deterioration seen on historic buildings and sculptures exposed to acid rain.
  • Calcium carbonate鈥檚 vulnerability to acid is due to its basic nature, which reacts with acids to neutralize them.
Protecting structures from acid rain involves understanding and managing these chemical interactions.
Acid Rain
Acid rain is the term used to describe rain that has a higher level of acidity than normal. It forms when pollutants like sulfur dioxide \(SO_2\) and nitrogen oxides \(NO_x\) mix with atmospheric water. This can lower the pH of rainwater, turning it into a weak acid.
  • The main contributor to acid rain is human activity, such as emissions from power plants and factories.
  • Acid rain can damage ecosystems, harming plants and aquatic life, as well as eroding buildings and monuments.
  • Mitigation strategies involve reducing emissions and using alternative energy sources.
Raising awareness about acid rain is crucial for protecting the environment and conserving cultural heritage.
Balance Chemical Equation
Balancing a chemical equation ensures that the same number of atoms are present on both sides of the equation. This reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.
  • In the reaction between sulfuric acid \(H_2SO_4\) and calcium carbonate \(CaCO_3\), the products are water \(H_2O\), carbon dioxide \(CO_2\), and calcium sulfate \(CaSO_4\).
  • The chemical equation is represented as: \( H_2SO_4 + CaCO_3 \rightarrow H_2O + CO_2 + CaSO_4 \).
  • This equation is already balanced, meaning it has equal numbers of hydrogen, sulfur, oxygen, calcium, and carbonate atoms on both sides.
Learning how to balance equations helps in understanding chemical reactions and ensuring accuracy in scientific calculations.

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Most popular questions from this chapter

Trace organic compounds in the atmosphere are first concentrated and then measured by gas chromatography. In the concentration step, several liters of air are pumped through a tube containing a porous substance that traps organic compounds. The tube is then connected to a gas chromatograph and heated to release the trapped compounds. The organic compounds are separated in the column and the amounts are measured. In an analysis for benzene and toluene in air, a 3.00-L sample of air at 748 torr and \(23^{\circ} \mathrm{C}\) was passed through the trap. The gas chromatography analysis showed that this air sample contained \(89.6\) ng benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) and \(153 \mathrm{ng}\) toluene \(\left(\mathrm{C}_{7} \mathrm{H}_{8}\right)\). Calculate the mixing ratio (see Exercise 121 ) and number of molecules per cubic centimeter for both benzene and toluene.

A gas sample containing \(1.50\) moles at \(25^{\circ} \mathrm{C}\) exerts a pressure of 400 . torr. Some gas is added to the same container and the temperature is increased to \(50 .{ }^{\circ} \mathrm{C}\). If the pressure increases to 800\. torr, how many moles of gas were added to the container? Assume a constant-volume container.

Consider two different containers, each filled with 2 moles of \(\mathrm{Ne}(\mathrm{g})\). One of the containers is rigid and has constant volume. The other container is flexible (like a balloon) and is capable of changing its volume to keep the external pressure and internal pressure equal to each other. If you raise the temperature in both containers, what happens to the pressure and density of the gas inside each container? Assume a constant external pressure.

A mixture of \(1.00 \mathrm{~g} \mathrm{H}_{2}\) and \(1.00 \mathrm{~g} \mathrm{He}\) is placed in a \(1.00-\mathrm{L}\) container at \(27^{\circ} \mathrm{C}\). Calculate the partial pressure of each gas and the total pressure.

Small quantities of hydrogen gas can be prepared in the laboratory by the addition of aqueous hydrochloric acid to metallic zinc. $$ \mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g) $$ Typically, the hydrogen gas is bubbled through water for collection and becomes saturated with water vapor. Suppose 240\. mL of hydrogen gas is collected at \(30 .{ }^{\circ} \mathrm{C}\) and has a total pressure of \(1.032\) atm by this process. What is the partial pressure of hydrogen gas in the sample? How many grams of zinc must have reacted to produce this quantity of hydrogen? (The vapor pressure of water is 32 torr at \(30^{\circ} \mathrm{C}\).)
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