Explanation Given: Mass of sample of dry ice , m C O 2 = 1.20 g Volume of the flask, V = 755 mL Pressure of N 2 = 725 m m H g Temperature, T = 25 o C = 25 + 273 .15 = 298 .15 K Explanation: The total pressure of the flask is given by P total = P N 2 + P CO 2 To find out the total pressure, pressure of C O 2 is to be calculated. To convert the given pressure of N 2 = 725 m m H g into atmospheres, use the following relation: ∵ 760 mmHg = 1 atm ∴ 725 mmHg = 1 atm × 725 mmHg 760 mmHg = 0.95395 atm Convert the given volume 755 mL into L by the use of following relation: 1 000 mL = 1 L ∴ 755 mL = 1 L × 755 mL 1000 mL = 0.755 L The number of moles of CO 2 is given by Number of moles ( n ) = Mass of CO 2 Molar mass of CO 2 Substitute mass of C O 2 = 1

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Chapter 5, Problem 63E

Interpretation Introduction

To determine: The total pressure present in the flask

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Chapter 5, Problem 62E

Chapter 5, Problem 64E

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Ch. 5 - Prob. 1SAQ Ch. 5 - Prob. 2SAQ Ch. 5 - Prob. 3SAQ Ch. 5 - Prob. 4SAQ Ch. 5 - Prob. 5SAQ Ch. 5 - Prob. 6SAQ Ch. 5 - Prob. 7SAQ Ch. 5 - Prob. 8SAQ Ch. 5 - Q9. A gas sample at STP contains 1.15 g oxygen and...Ch. 5 - Prob. 10SAQ

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