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Chapter 5: Problem 41

Some chambers used to grow bacteria that thrive on \(\mathrm{CO}_{2}\) have a gas mixture consisting of \(95.0 \% \mathrm{CO}_{2}\) and \(5.0 \% \mathrm{O}_{2}\) (mole percent). What is the partial pressure of each gas if the total pressure is \(735 \mathrm{~mm} \mathrm{Hg}\) ?

Short Answer

Expert verified
Answer: The partial pressure of CO2 in the gas mixture is 698.25 mm Hg, and the partial pressure of O2 is 36.75 mm Hg.

Step by step solution

01

Calculate the mole fractions of each gas

Mole fraction is given as a percentage in this problem. Convert these percentages into fractions by dividing the percentage by 100. - mole fraction of CO2 = 95.0% / 100 = 0.95 - mole fraction of O2 = 5.0% / 100 = 0.05
02

Calculate partial pressure of each gas

Use the formula for partial pressure: Partial pressure = mole fraction * total pressure Calculate the partial pressure for CO2 and O2 separately: Partial pressure of CO2 = 0.95 * 735 mm Hg = 698.25 mm Hg Partial pressure of O2 = 0.05 * 735 mm Hg = 36.75 mm Hg
03

Present the results

The partial pressure of CO2 in the gas mixture is 698.25 mm Hg, and the partial pressure of O2 is 36.75 mm Hg.

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Most popular questions from this chapter

Nitroglycerine is an explosive used by the mining industry. It detonates according to the following equation: $$ 4 \mathrm{C}_{3} \mathrm{H}_{5} \mathrm{~N}_{3} \mathrm{O}_{9}(l) \longrightarrow 12 \mathrm{CO}_{2}(g)+6 \mathrm{~N}_{2}(g)+10 \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{O}_{2}(g) $$ What volume is occupied by the gases produced when \(10.00 \mathrm{~g}\) of nitroglycerine explodes? 'The total pressure is \(1.45 \mathrm{~atm}\) at \(523^{\circ} \mathrm{C}\).

Ammonium nitrate can be used as an effective explosive because it decomposes into a large number of gaseous products. At a sufficiently high temperature, ammonium nitrate decomposes into nitrogen, oxygen, and steam. (a) Write a balanced equation for the decomposition of ammonium nitrate. (b) If \(1.00 \mathrm{~kg}\) of ammonium nitrate is sealed into a \(50.0\) - \(\mathrm{L}\) steel drum and heated to \(787^{\circ} \mathrm{C}\), what is the pressure in the drum, assuming \(100 \%\) decomposition?

Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At \(755 \mathrm{~mm} \mathrm{Hg}\) and \(25^{\circ} \mathrm{C}\), it has a density of \(1.71 \mathrm{~g} / \mathrm{L}\). (a) What is the molar mass of cyclopropane? (b) Cyclopropane is made up of \(85.7 \% \mathrm{C}\) and \(14.3 \% \mathrm{H}\). What is the molecular formula of cyclopropane?

A gas effuses \(1.55\) times faster than propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) at the same temperature and pressure. (a) Is the gas heavier or lighter than propane? (b) What is the molar mass of the gas?

An intermediate reaction used in the production of nitrogencontaining fertilizers is that between ammonia and oxygen: $$ 4 \mathrm{NH}_{3}(\mathrm{~g})+5 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) $$ A \(150.0\) - \(\mathrm{L}\) reaction chamber is charged with reactants to the following partial pressures at \(500^{\circ} \mathrm{C}: P_{\mathrm{NH}_{3}}=1.3 \mathrm{~atm}, P_{\mathrm{O}_{2}}=1.5 \mathrm{~atm} .\) What is the limiting reactant?
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