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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 (H₂O), carbon dioxide (CO₂), and calcium sulfate (CaSO₄).

Step by step solution

01

Identify the reactants

The reactants in this reaction are sulfuric acid (H₂SO₄) and calcium carbonate (CaCO₃). 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 (H₂O), carbon dioxide (CO₂), and calcium sulfate (CaSO₄) are formed as products.
03

Write the unbalanced equation

Now we can write the unbalanced chemical equation: H₂SO₄ + CaCO₃ → H₂O + CO₂ + CaSO₄
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: H₂SO₄ + CaCO₃ → H₂O + CO₂ + CaSO₄ 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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Most popular questions from this chapter

A piece of solid carbon dioxide, with a mass of \(7.8 \mathrm{~g}\), is placed in a 4.0-L otherwise empty container at \(27^{\circ} \mathrm{C}\). What is the pressure in the container after all the carbon dioxide vaporizes? If \(7.8 \mathrm{~g}\) solid carbon dioxide were placed in the same container but it already contained air at 740 torr, what would be the partial pressure of carbon dioxide and the total pressure in the container after the carbon dioxide vaporizes?

The average lung capacity of a human is \(6.0 \mathrm{~L}\). How many moles of air are in your lungs when you are in the following situations? a. At sea level \((T=298 \mathrm{~K}, P=1.00 \mathrm{~atm})\). b. \(10 . \mathrm{m}\) below water \((T=298 \mathrm{~K}, P=1.97 \mathrm{~atm})\). c. At the top of Mount Everest \((T=200 . \mathrm{K}, P=0.296 \mathrm{~atm})\).

An organic compound containing only C, H, and N yields the following data. i. Complete combustion of \(35.0 \mathrm{mg}\) of the compound produced \(33.5 \mathrm{mg} \mathrm{CO}_{2}\) and \(41.1 \mathrm{mg} \mathrm{H}_{2} \mathrm{O}\). ii. A \(65.2\) -mg sample of the compound was analyzed for nitrogen by the Dumas method (see Exercise 129), giving \(35.6 \mathrm{~mL}\) of dry \(\mathrm{N}_{2}\) at 740 . torr and \(25^{\circ} \mathrm{C}\). iii. The effusion rate of the compound as a gas was measured and found to be \(24.6 \mathrm{~mL} / \mathrm{min}\). The effusion rate of argon gas, under identical conditions, is \(26.4 \mathrm{~mL} / \mathrm{min}\). What is the molecular formula of the compound?

A mixture of chromium and zinc weighing \(0.362 \mathrm{~g}\) was reacted with an excess of hydrochloric acid. After all the metals in the mixture reacted, \(225 \mathrm{~mL}\) dry of hydrogen gas was collected at \(27^{\circ} \mathrm{C}\) and 750 . torr. Determine the mass percent of \(\mathrm{Zn}\) in the metal sample. [Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas; chromium reacts with hydrochloric acid to produce chromium(III) chloride and hydrogen gas.]

In 1897 the Swedish explorer Andreé tried to reach the North Pole in a balloon. The balloon was filled with hydrogen gas. The hydrogen gas was prepared from iron splints and diluted sulfuric acid. The reaction is $$ \mathrm{Fe}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{FeSO}_{4}(a q)+\mathrm{H}_{2}(g) $$ The volume of the balloon was \(4800 \mathrm{~m}^{3}\) and the loss of hydrogen gas during filling was estimated at \(20 . \%\). What mass of iron splints and \(98 \%\) (by mass) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) were needed to ensure the complete filling of the balloon? Assume a temperature of \(0^{\circ} \mathrm{C}\), a pressure of \(1.0\) atm during filling, and \(100 \%\) yield.
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