A 7.00 L tank at 12.4 °C is filled with 19.4 g of sulfur tetrafluoride gas and 10.3 g of dinitrogen difluoride gas. You can assume both gases behar gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas mole fraction sulfur tetrafluoride dinitrogen difluoride

A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas is measured to be 155. kPa. The piston is now pushed down, compressing the gas, until the gas has a final volume of 5.10 L. Calculate the final pressure of the gas. Round your answer to 3 significant digits. piston cylinder gas O kPa

According to Charles’s law, the volume of a gas is directly related to its temperature in kelvins at constant pressure and the number of moles. In your initial post to the discussion, respond to the following prompts: What if there was an inverse relationship between the temperature and the volume? How do you think the world might be different? How would this change our day-to-day lives? Pick one of the following questions and try to answer it using one of the laws you learned in this module: How do spray cans work? Why do you need to fill up your tires with air on a cold day? Why do soda cans explode? When you inhale, your diaphragm increases in volume. How does this allow you to breathe? How does a syringe fill? How does filling a basketball with air increase its volume?

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

A 10.00 L tank at 12.8 °C is filled with 19.2 g of carbon dioxide gas and 15,7 g of dinitrogen monoxide 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. carbon dioxide dinitrogen monoxide mole fraction 0 0

A gas sample containing only BF3, SO2 and S2F2 has the following mass percent composition: 44.3% BF3 and 13.3% SO2. Calculate the partial pressure (torr) of SO2 if the total pressure of the sample is 1.90 atm.

Consider the apparatus shown below with the valve closed. The volume and pressure of each gas is indicated. F2 N2 Valve 3.00 L 6.00 L 2.00 atm 4.00 atm When the valve is opened the two gases mix uniformly. At that point, what is the mole fraction of nitrogen in the mixture? 0.800 none of the answers are correct 0.500 0.333