Compare the masses of a one-liter sample of hydrogen and a one-liter sample of helium gas, each at 25°C and 5.0 atm pressure. A) The helium gas has twice the mass of the hydrogen gas. B) The helium gas has four times the mass of the hydrogen gas. C) The hydrogen gas has twice the mass of the helium gas. D) The hydrogen gas has four times the mass of the helium gas. E) The mass of the hydrogen gas equals the mass of the helium gas.

2. During the experiment, you collect the following data: Mass of flask: 80.001 Mass of flask + unknown condensed liquid: 80.452 Temperature of water bath: 100 °C Pressure of gas in our system: 0.998 atm Volume of gas in our system: 265 mL How many moles of gas were produced? Hint: Do not forget to convert units as needed. Group of answer choices: A) 0.00864 moles B) 32.2 moles C) 0.0322 moles D) 8.64 moles

Use the References to access important values if needed for this question. A sample of hydrogen gas has a density of g/L at a pressure of 1.20 atm and a temperature of 53 °C. Assume ideal behavior. Submit Answer Retry Entire Group 9 more group attempts remaining

Without working the math, use reasoning and logic about molar volume at STP to answer the question.

[Review Topics] [References] Use the References to access important values if needed for this question. A 0.380 gram sample of hydrogen gas has a volume of 834 milliliters at a pressure of 3.48 atm. The temperature of the H₂ gas sample is °C.

Use the following information to determine how many moles were produced? Round to two decimal places. Remember: for ideal gas law, you may need to convert multiple units. Pressure: = 742.1 mm HgVolume = 9.65 LTemperature = 45.5 °C

Please answer the following True or Flase statement: Volume of a gas is directly proportional to the mass of the gass, not the number of moles. (True or False?