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Chapter 1: Problem 78

Tums is a popular remedy for acid indigestion. A typical Tums tablet contains calcium carbonate plus some inert substances. When ingested, it reacts with the gastric juice (hydrochloric acid) in the stomach to give off carbon dioxide gas. When a 1.328 -g tablet reacted with \(40.00 \mathrm{~mL}\) of hydrochloric acid (density: \(1.140 \mathrm{~g} / \mathrm{mL}\) ), carbon dioxide gas was given off and the resulting solution weighed 46.699 g. Calculate the number of liters of carbon dioxide gas released if its density is \(1.81 \mathrm{~g} / \mathrm{L}\).

Short Answer

Expert verified
The volume of carbon dioxide gas released is approximately 0.126 Liters.

Step by step solution

01

Calculate the mass of reactants

The mass of reactants consists of the Tums tablet and Hydrochloric acid:The mass of Tums tablet is given as 1.328g.The volume of Hydrochloric acid is given as 40.00mL, with a density of 1.140g/mL. Multiply the volume with the density to get the mass. Thus, the mass of Hydrochloric acid is: \(40.00 \mathrm{~mL} * 1.140 \mathrm{~g/mL} = 45.60g\)Add these together to get the total mass of reactants: \(1.328g + 45.60g = 46.928g\).
02

Calculate the mass of Carbon Dioxide gas

By the Law of Conservation of Mass, mass of reactants equals mass of products. Hence, subtract the weight of resulting solution from the total mass of reactants to get the mass of Carbon Dioxide gas: Mass of Carbon Dioxide gas = mass of reactants - mass of resulting solution = \(46.928g - 46.699g = 0.229g\)
03

Calculate the volume of Carbon Dioxide gas

The density of Carbon Dioxide gas is given to be \(1.81 \mathrm{~g/L}\). We can use this to find the volume of CO2 gas released using the formula: volume = mass/density. Divide the mass of CO2 calculated in Step2 by the density of CO2. Thus, volume of Carbon Dioxide gas = \(0.229g / 1.81 \mathrm{~g/L} \approx 0.126 \mathrm{~L}\)

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Most popular questions from this chapter

One gallon of gasoline burned in an automobile's engine produces on the average \(9.5 \mathrm{~kg}\) of carbon dioxide, which is a greenhouse gas, that is, it promotes the warming of Earth's atmosphere. Calculate the annual production of carbon dioxide in kilograms if there are 40 million cars in the United States, and each car covers a distance of \(5000 \mathrm{mi}\) at a consumption rate of 20 mi per gallon.

A 250 -mL glass bottle was filled with 242 mL of water at \(20^{\circ} \mathrm{C}\) and tightly capped. It was then left outdoors overnight, where the average temperature was \(-5^{\circ} \mathrm{C}\). Predict what would happen. The density of water at \(20^{\circ} \mathrm{C}\) is \(0.998 \mathrm{~g} / \mathrm{cm}^{3}\) and that of ice at \(-5^{\circ} \mathrm{C}\) is \(0.916 \mathrm{~g} / \mathrm{cm}^{3}\)

Chlorine is used to disinfect swimming pools. The accepted concentration for this purpose is 1 ppm chlorine or \(1 \mathrm{~g}\) of chlorine per million \(\mathrm{g}\) of water. Calculate the volume of a chlorine solution (in milliliters) a homeowner should add to her swimming pool if the solution contains 6.0 percent chlorine by mass and there are \(2 \times 10^{4}\) gallons of water in the pool. (1 gallon \(=3.79 \mathrm{~L}\); density of liquids \(=1.0 \mathrm{~g} / \mathrm{mL} .)\)

The total volume of seawater is \(1.5 \times 10^{21} \mathrm{~L}\). Assume that seawater contains 3.1 percent sodium chloride by mass and that its density is \(1.03 \mathrm{~g} / \mathrm{mL}\). Calculate the total mass of sodium chloride in kilograms and in tons. \((1\) ton \(=2000 \mathrm{lb} ; 1 \mathrm{lb}=453.6 \mathrm{~g} .)\).

Do these statements describe chemical or physical properties? (a) Oxygen gas supports combustion. (b) Fertilizers help to increase agricultural production. (c) Water boils below \(100^{\circ} \mathrm{C}\) on top of a mountain. (d) Lead is denser than aluminum. (e) Uranium is a radioactive element.
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