A sample of gas at 4.0atm and 25.0mL is heated from 25°C to 40°C. If the pressure remains constant, what is the final volume of the gas? O 40.0mL O 23.8mL O 26.2mL O 25.0mL

2.0 g of H2 gas and 4.0 g of He gas are contained in a 50.0-L gas-tight vessel 25.0o C. Calculate the partial pressure of each gas.

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A 6.00 L tank at -2.4 °C is filled with 2.01 g of sulfur tetrafluoride gas and 6.11 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas sulfur tetrafluoride sulfur hexafluoride mole fraction 0 0 X Ś 0 000 13 Ar

MI < CO C. Under identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through identical membranes simultaneously. After a certain amount of time, it was found that 5.75 mL of O2 had passed through the membrane, but only 3.86 mL of of the unknown gas had passed through. What is the molar mass of the unknown gas? unknown molar mass: g/mol MacBook Pro The %23 %$4 delet 4. 5. 3. R. P. H. K. B. MOSISO command uondo

A gas has a density of 1.53 g L-1 at 53 °C and P = 0.938 atm. What will be its density at 161 °C? Calculate the molar mass of the gas, assuming it obeys the ideal gas law.Density at 161 °C =  g L-1Molar mass =  g mol-1

An unknown gas at 79.1 ∘C and 1.10 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior, what is the density of the gas? density:                                                g/L

BIOL 1603: Org & Evol - Google x A ALEKS - Katie Matthews - Grac x Content app.101edu.co → C esc 1 F1 A glass container was initially charged with 1.50 moles of a gas sample at 5.00 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 33.1 °C, so the final pressure in the container was reduced to 1.50 atm. How many moles of the gas sample are present at the end? Q 2 F2 W # 3 80 E $ 4 F4 R % 675 뽀 F5 T 6 X Question 38 of 66 F6 Y Aktiv Chemistry & 7 F7 U * 00 8 DII F8 ( 1 9 X a Amazon.com: wireles F9 0 1 2 4 7 +/- 0 7 F10 5 8 P

The gas of a certain volcano had the following composition in mole percent: 60.0% CO2, 28.0% H2, 7.40% HCl, 1.80% HF, 2.70% SO2, and 0.100% H2S.  What would be the partial pressure of  HF in atmospheres if the total pressure was 285 mmHg? 1atm = 760mmHg