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8. (a) A 50.0 g sample occupies 11.2 L at STP. Calculate the molecular weight of this gas. (R = 0.0821 L atm K- mol-)

8. (a) A 50.0 g sample occupies 11.2 L at STP. Calculate the molecular weight of this gas. (R = 0.0821 L atm K- mol-)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question 8.(a)
6. Suppose a balloon is launched whon the temperature is 22.5 °C and the barometric pressure is 754.0 mm Hg. If the balloon's initial volume is 4.19 x 10' L, what will the volume be at a height of 20 miles where the pressure is 76.0 mm Hg and the temperature is-33.0 °C? 7. (a) If 0.2 mol of helium occupies a volume of 64,0 L at a pressure of 0.15 atm, what is the temperature of the gas? (R 0.0821 L atm K'mol') (b) A flashbulb of volume 2.6 cm³ contains O2(g) at a pressure of 2.3 atm and a temperature of 26 °C. How many moles of O2(g) does the flashbulb contain? (R = 0.0821 L atm K-'mol') M=MRT 8. (a) A 50.0 g sample occupies 11.2 L at STP. Calculate the molecular weight of this gas. (R = 0.0821 L atm K' mol-') (b) At STP, a sample of oxygen gas occupies a volume of Calculate the mass o oxygen gas in the sample. (R = 0.0821 L atm K-'mol, RAM: 0 = 16.0) (c) An amount of 8.8 g of CO2 is filled inside a 100,0 container at a temperature C 27.0 °C. What will be the pressure (in Pascal) in the container? (R = 8.314 J K' mol, Molar masas: CO2 = 44.0 g mol') (d) Calculate the density of CO2 at 1200 Pa and 20°C. (R = 0.0821 L atm K mol', Molar mass: CO2 = 44.0 g mol') 9.) (a) Calculate the pressure of gas, in atm, if 8.25 x 10 mol occupies a volume of 174.0 m at -24.0 °C. (R= 0.0821 L atm K mol) (b) A deep breath of air has a volume of 1.05 L at a pressure of 740 mm Hg and body temperature of 37 °C. Calculate the number of molecules in the breath. (R = 0.0821 L atm K- mol) T Acm oundaonS die
Transcribed Image Text:6. Suppose a balloon is launched whon the temperature is 22.5 °C and the barometric pressure is 754.0 mm Hg. If the balloon's initial volume is 4.19 x 10' L, what will the volume be at a height of 20 miles where the pressure is 76.0 mm Hg and the temperature is-33.0 °C? 7. (a) If 0.2 mol of helium occupies a volume of 64,0 L at a pressure of 0.15 atm, what is the temperature of the gas? (R 0.0821 L atm K'mol') (b) A flashbulb of volume 2.6 cm³ contains O2(g) at a pressure of 2.3 atm and a temperature of 26 °C. How many moles of O2(g) does the flashbulb contain? (R = 0.0821 L atm K-'mol') M=MRT 8. (a) A 50.0 g sample occupies 11.2 L at STP. Calculate the molecular weight of this gas. (R = 0.0821 L atm K' mol-') (b) At STP, a sample of oxygen gas occupies a volume of Calculate the mass o oxygen gas in the sample. (R = 0.0821 L atm K-'mol, RAM: 0 = 16.0) (c) An amount of 8.8 g of CO2 is filled inside a 100,0 container at a temperature C 27.0 °C. What will be the pressure (in Pascal) in the container? (R = 8.314 J K' mol, Molar masas: CO2 = 44.0 g mol') (d) Calculate the density of CO2 at 1200 Pa and 20°C. (R = 0.0821 L atm K mol', Molar mass: CO2 = 44.0 g mol') 9.) (a) Calculate the pressure of gas, in atm, if 8.25 x 10 mol occupies a volume of 174.0 m at -24.0 °C. (R= 0.0821 L atm K mol) (b) A deep breath of air has a volume of 1.05 L at a pressure of 740 mm Hg and body temperature of 37 °C. Calculate the number of molecules in the breath. (R = 0.0821 L atm K- mol) T Acm oundaonS die
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