A gas sample occupies a volume of 150 mL at a temperature of 296 K and a pressure of 0.969 atm. How many moles of gas are there? Show your work. Answer using a complete sentence. Don't forget to change mL to L.

1. At 27°C and 720 Torr, a certain gas sample has a volume of 765 mL. a. What would be its new volume if the temperature and pressure were changed to 57°C and 792 Torr? Hint: Use Combined Gas Law. b. How many moles are present in that gas sample? Hint: Use Universal Gas Law.

How many gas molecules are present in 727 mL of propane (C3H8) at 27 °C and 494 torr pressure? Enter using scientific notation. How many atoms are present? Enter using scientific notation. What would the volume of the sample be at STP? Enter using decimal notation.

Sulfur hexafluoride gas is collected at 3.0 °C in an evacuated flask with a measured volume of 30.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.270 atm . Calculate the mass and number of moles of sulfur hexafluoride gas that were collected. Round your answer to 3 significant digits. mass: mole: mol

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

A balloon contains 0.154 mol of gas and has a volume of 2.61 L . If an additional 0.200 mol of gas is added to the balloon (at the same temperature and pressure), what will its final volume be? Express your answer in liters to three significant figures.

A gas sample initially at 1 atm increases in pressure to 4.51 atm as the volume shrinks to 5.6 L. What was the initial volume? Show work on your paper. In the box below, enter your numeric answer only.

When 5.5 g sodium reacts with an excess of sulfuric acid at 32°C, what pressure of hydrogen gas will result in a 500.0 mL container?