A sample of hydrogen gas occupies a volume of 8.54 L at 55.0°C and 0.450 atm. If it is desired to decrease the volume of the gas sample to 7.50 L, while increasing its pressure to 0.612 atm, the temperature of the gas sample at the new volume and pressure must be __________°C.

Using the combined gas law

What is the molar mass of an unknown gas with a density of 1.90 g/L at 1.00 atm and 25.0 °C?   ____g/mol?

A sample of krypton gas occupies a volume of 7.85 L at 53.0°C and 0.510 atm. If it is desired to increase the volume of the gas sample to 9.40 L, while decreasing its pressure to 0.336 atm, the temperature of the gas sample at the new volume and pressure must be °C.

A gas that has a volume of 8.5 liters, a temperature of 35 0C, and an unknown pressure has its volume increased to 17 liters and its temperature decreased to 130C.  If I measure the pressure after the change to be 1.6 atm, what was the original pressure of the gas? If I have 3.6 liters of gas at a temperature of 36 0C and a pressure of 4.6 atm, what will be the pressure of the gas if I raise the temperature to 84 0C and decrease the volume to 2.6 liters? A tire has a pressure of 1.4 atm and 21 0C.  At the end of a long trip, the tire pressure increased to 1.6 atm.  What is the new temperature inside of the tire in degrees Celsius? A sample of chlorine gas is under a 1.24 atm pressure, in a 2.84 L container, at 110 0C .  How many grams of chlorine are present in this sample?

Calculating partial pressure in a gas mixture tab A 7.00 L tank at 25.3 °C is filled with 6.94 g of carbon dioxide gas and 3.83 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. carbon dioxide caps lock chlorine pentafluoride Explanation Esc ! Check Type here to search. 1 Total pressure in tank: F1 Q mole fraction: partial pressure: A mole fraction: partial pressure: S @ 2 F2 W S F3 # #m 81 3 E 0x D 0 atm 0 atm atm $ 4 R F5 % 5 LL X F 20 F6 T A 3 6 G 8 F7 & Y 7 2 H FB © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center ^ d 63°F Mostly cloudy ★ 8 U 4 FO J ( Collector v2. prt sc 9 1 F10 5 home 1 K O 01 M athenaCollector v2... 2 15 F12 P L veert 2:36 PM 11/13/2023 = I All Bookmarks Danasia V do Accessibility ? & ☐ Calehe backspace 1 MISKESS doscop mm 740

A container is filled with an ideal gas to a pressure of 12.5 atm at 0°C. What will be the pressure in the container if it is heated to 40.°C? Pressure =                   atm At what temperature would the pressure be 5.00 atm? Temperature =                    K At what temperature would the pressure be 25.3 atm? Temperature =                    K

A sample of krypton gas at a pressure of 0.777 atm and a temperature of 285 °C, occupies a volume of 609 mL. If the gas is cooled at constant pressure until its volume is 522 mL, the temperature of the gas sample will be °C.

A sample of an ideal gas has a volume of 3.40 L at 10.80 °C and 1.80 atm. What is the volume of the gas at 19.20 °C and 0.986 atm? V = L

17 . A 40.0 L weather balloon is filled with air at sea level where the pressure is 1.0 atm and 15 °C.  What will be the volume of the weather balloon, in L, at 6000 feet elevation where the pressure is 1.239 atm and 4.0 oC? 18. An empty 2.00 L soda bottle is filled with 31.89 grams of gaseous CO2.  Calculate the temperature, in oC, at which the bottle will explode if the maximum pressure the bottle can hold is about 10.2 atm. 19. A flask of volume 3.21 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.7 °C.  What mass of sodium is required to completely react with the chlorine gas to make sodium chloride?  Assume the reaction goes to completion and there is no limiting reagent.  Hint: calculate the moles of Cl2 gas in the flask first. (Do not put units in answer) 2 Na (s) + Cl2 (g) --> 2 NaCl (s)