   # A halothane-oxygen mixture (C 2 HBrCIF 3 + O 2 ) can be used as an anesthetic. A tank containing such a mixture has the following partial pressures: P (halothane) = 170 mm Hg and P (O 2 ) = 570 mm Hg. (a) What is the ratio of the number of moles of halothane to the number of moles of O 2 ? (b) If the tank contains 160 g of O 2 , what mass of C 2 HBrCIF 3 is present? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 10, Problem 39PS
Textbook Problem
568 views

## A halothane-oxygen mixture (C2HBrCIF3 + O2) can be used as an anesthetic. A tank containing such a mixture has the following partial pressures: P (halothane) = 170 mm Hg and P (O2) = 570 mm Hg. (a) What is the ratio of the number of moles of halothane to the number of moles of O2? (b) If the tank contains 160 g of O2, what mass of C2HBrCIF3 is present?

(a)

Interpretation Introduction

Interpretation:

The ratio of number of moles of halothane vapour to oxygen gas and mass of C2HBrClF3 has to be given.

Concept Introduction:

• Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
• Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
• Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

xa=nantotal

• pa=xa×Ptotal

Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

### Explanation of Solution

Given:

p(halothane)=170mmHgp(O2)=570mmHg

Total pressure can be found out by taking the sum of these two partial pressures.

Totalpressure=570mmHg+170mmHg=740mmHg

Now we can calculate the mole fraction by the equation

pa=xa×Ptotalxa=paPtotal

xhalothane=170mmHg740mmHg=0

(b)

Interpretation Introduction

Interpretation:

The ratio of number of moles of halothane vapour to oxygen gas and mass of C2HBrClF3 has to be given.

Concept Introduction:

• Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
• Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
• Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

xa=nantotal

• pa=xa×Ptotal

Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

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