Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 52

A person accidentally swallows a drop of liquid oxygen, \(\mathrm{O}_{2}(l)\), which has a density of \(1.149 \mathrm{~g} / \mathrm{mL}\). Assuming the drop has a volume of \(0.050 \mathrm{~mL}\), what volume of gas will be produced in the person's stomach at body temperature \(\left(37^{\circ} \mathrm{C}\right)\) and a pressure of \(1.0 \mathrm{~atm}\) ?

Short Answer

Expert verified
The volume of O₂ gas produced in the person's stomach at body temperature (37°C) and a pressure of 1.0 atm will be 45.7 mL.

Step by step solution

01

Finding the mass of liquid oxygen drop

We are given the density of the liquid oxygen drop, which is 1.149 g/mL, and its volume, which is 0.050 mL. We will use these values to find the mass of this drop. Mass = Density × Volume.
02

Calculate the mass of the liquid oxygen

We plug the values we have into the formula from Step 1: \( Mass = (1.149 \frac{g}{mL}) \times (0.050 mL) \) By multiplying the values, we get: \( Mass = 0.05745 \ g \)
03

Finding the number of moles of O₂

Now that we have the mass of the liquid oxygen, we will find the number of moles of O₂. We know the molar mass of O₂ is 32.00 g/mol. We will use the formula: Moles of O₂ = (mass of O₂) / (molar mass of O₂)
04

Calculate the number of moles of O₂

Plugging in the values from Step 2 and the molar mass of O₂, we get: \( Moles \ of \ O_{2} = \frac{0.05745 \ g}{32.00 \frac{g}{mol}} \) By dividing the mass by molar mass, we get: \( Moles \ of \ O_{2} = 0.0018 \ mol \)
05

Find the volume of O₂ gas using the ideal gas law

We have the number of moles of O₂ gas and we are given the pressure (1.0 atm) and temperature (37°C or 310 K). The ideal gas law formula is: \(PV = nRT\) Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L atm /(K mol)), and T is the temperature in Kelvin. We will solve for V (volume of gas).
06

Calculate the volume of O₂ gas

Plug in the values we have for P, n, R, and T, and solve for V: \( V = \frac{nRT}{P} \\ V = \frac{(0.0018 \ mol)(0.0821 \frac{L \cdot atm}{K \cdot mol})(310 \ K)}{1.0 \ atm} \) By multiplying and dividing the values, we get: \( V = 0.0457 \ L \)
07

Express the result in mL

We will convert the volume of O₂ gas from liters to milliliters by multiplying by 1000: Volume of O₂ gas = 0.0457 L × 1000 mL/L Volume of O₂ gas = 45.7 mL Thus, the volume of O₂ gas produced in the person's stomach at body temperature (37°C) and a pressure of 1.0 atm will be 45.7 mL.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

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 \(0^{\circ} \mathrm{C}, \mathrm{a}\) pressure of \(1.0\) atm during filling, and \(100 \%\) yield.

Sulfur trioxide, \(\mathrm{SO}_{3}\), is produced in enormous quantities each year for use in the synthesis of sulfuric acid. $$ \begin{aligned} \mathrm{S}(s)+\mathrm{O}_{2}(g) & \longrightarrow \mathrm{SO}_{2}(g) \\ 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{SO}_{3}(g) \end{aligned} $$ What volume of \(\mathrm{O}_{2}(g)\) at \(350 .{ }^{\circ} \mathrm{C}\) and a pressure of \(5.25 \mathrm{~atm}\) is needed to completely convert \(5.00 \mathrm{~g}\) sulfur to sulfur trioxide?

The steel reaction vessel of a bomb calorimeter, which has a volume of \(75.0 \mathrm{~mL}\), is charged with oxygen gas to a pressure of 145 atm at \(22^{\circ} \mathrm{C}\). Calculate the moles of oxygen in the reaction vessel.

A 2.50-L container is filled with \(175 \mathrm{~g}\) argon. a. If the pressure is \(10.0\) atm, what is the temperature? b. If the temperature is \(225 \mathrm{~K}\), what is the pressure?

Write reactions to show how nitric and sulfuric acids are produced in the atmosphere.
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation

Chemistry Branches

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free