For an ideal gas, calculate the following quantities. (a) The pressure of the gas if 0.155 mol occupies 217 mL at 35°C. 18.06 atm (b) The temperature (in kelvins) at which 0.0290 mol occupies 1.00 L at 0.553 atm. 235.9 ♥K (c) The number of moles in 4.50 L at -1°C and 745 torr. Remember 1atm = 760 torr. 0.176 x mol (d) The volume occupied by 8.72 x 10-3 mol at 30.°C and a pressure of 1.37 kPa. Remember 1 atm = 101.325 kPa 1.60 X L

For an ideal gas, calculate the following quantities. (a) The pressure of the gas if 0.155 mol occupies 217 mL at 35°C. 18.06 atm (b) The temperature (in kelvins) at which 0.0290 mol occupies 1.00 L at 0.553 atm. 235.9 ♥K (c) The number of moles in 4.50 L at -1°C and 745 torr. Remember 1atm = 760 torr. 0.176 x mol (d) The volume occupied by 8.72 x 10-3 mol at 30.°C and a pressure of 1.37 kPa. Remember 1 atm = 101.325 kPa 1.60 X L

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter5: Gases, Liquids, And Solids

Section: Chapter Questions

Problem 5.33P: 5-33 A certain quantity of helium gas is at a temperature of 27 °C and a pressure of 1.00 atm. What...

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