There are 2 grams of H2 gas in a fixed volume container at 273 °C. 16 grams of He gas is added to the container and the temperature is raised to 819 °C. So what is the ratio of final pressure to initial pressure?    A) 12  B) 10  C) 5  D) 0.5  E) 4

4. A pressurized gas is allowed to expand. If the gas originally occupied a volume of 420 mL at a pressure of 300. psi, what volume will it occupy if the pressure is lowered to 125 psi?

4. A glass container was initially charged with 2.00 moles of a gas sample at 3.75 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 28.1 °C, so the final pressure in the container was reduced to 0.998 atm. Assume the volume stayed the same. How many moles of the gas sample are present at the end?

5] A 67.5 grams sample of sulfur dioxide gas was measured at 35.0*C with a volume of 3.67 L. Calculate the pressure of the gas. 6] A mixture of nitrogen, oxygen and ammonia have a total pressure of 235 kPa. If the pressure of nitrogen is 97.0 kPa and oxygen is 106 kPa, what is the partial pressure of the ammonia? 7] A container has a mixture of nitrogen gas and sulfur trioxide gas. Which will effuse faster and by what ratio? 8] A gas has a solubility in water of 16.9 grams/L at 15.0*C and 505 kPa of pressure. What is the solubility in water at 15.0*C and 606 kPa of pressure? 9] How many grams of calcium hydroxide are needed to produce 5.00 x 10² ml of a 1.66 M calcium hydroxide solution?

(Incorrect) Consider the reaction below P4(g) + 6 Cl₂(g) → 4 PC13(g) If 0.246 moles of P4 is mixed with 0.354 moles of Cl₂ in a 9.77-L rigid reaction vessel, what is the final pressure in the vessel after the reaction goes to completion? The final temperature is 350. °C. Assume 100% yield. 2.89 atm 1.24 atm (Your answer) 0.694 atm 2.21 atm (Correct answer) 5.15 atm

A sample of helium gas at 283 K and 0.736 atm occupies a volume of 4.08 L. If the pressure of the gas is increased, while at the same time it is heated to a higher temperature, the final gas volume A) could be larger or smaller than 4.08 L depending on the final pressure and temperature. B) will be smaller than 4.08 L. C) will be larger than 4.08 L.

.) A sample of nitrogen gas initially occupies a volume of 27.5 L at a temperature of 22.5 \deg C and a pressure of 3.25 atm. Calculate the sample's temperature (in \deg C) after the volume of the sample increases to 98.6 L and its pressure decreases to 1.75 atm. 1.