1. A balloon was filled to a volume of 2.50 L when the temperature was 30.0∘C. What would the volume become if the temperature dropped to 11.0∘C. 2. The surface temperature of Venus is about 1050 K, and the pressure is about 75 Earth atmospheres. Assuming that these conditions represent a Venusian "STP," what is the standard molar volume in liters of a gas on Venus?

2.00L of carbon dioxide gas (the main component of the Martian atmosphere) is contained at a pressure of 101.3 kPa at room temperature (21oC) on Earth. The daytime temperature at the equator during summer on Mars is also 21oC. If the atmospheric pressure on Mars is 6.01 mmHg, what volume would the gas occupy on Mars?

The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4240 L of hydrogen gas at STP, heat the mixture to run the reaction, then separate the ammonia from the reaction mixture. What volume of reactant, measured at STP, is left over? Assume the reaction goes to completion. N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)

A.) What is the temperature of 0.45 mol of gas at a pressure of 1.0 atm and a volume of 12.0 L ? Express the temperature in kelvins to two significant figures.   B.) A weather balloon is inflated to a volume of 25.9 L at a pressure of 752 mmHg and a temperature of 27.5∘C. The balloon rises in the atmosphere to an altitude where the pressure is 400. mmHg and the temperature is -15.3∘C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

7. Aluminum metal reacts with hydrochloric acid to produce hydrogen gas. 2 Al (s) + 6 HCl (aq) --> 2 AlCl3 (aq) + 3 H2 (g) If 2.3 L of H2 was collected over water at 25.0 oC and 568.5 mmHg, x grams of aluminum must have reacted with excess hydrochloric acid. What is the value of x? The partial pressure of water at 25.0 oC is 23.8 mmHg.

4. In a laparoscopic surgery, carbon dioxide gas is used to inflate the abdomen to separate the internal organs and the abdominal wall. If the CO2 injected into the abdomen produces a pressure of 17 mmHg and a volume of 2.9 L at 26°C, how many moles of CO2 were used? How many grams? 5. What is the total pressure, in millimeters of mercury, of a gas mixture containing krypton gas at 0.45 atm and neon gas at 650 mmHg?

A helium-filled weather balloon has a volume of 731 L at 23.9°C and 754 mmHg. It is released and rises to an altitude of 2.07 km, where the pressure is 641 mmHg and the temperature is 9.9°C. a. The volume of the balloon at this altitude is  L.       2.  A sample of helium gas at a pressure of 761 mmhg and a temperature of 32ºc, occupies a volume of 8.71 L. If the gas is cooled at constant pressure to a temperature of 11ºc, the volume of the gas sample will be   L.

A piece of dry ice (solid carbon dioxide) with a mass of 25.5 g sublimes (converts from solid to gas) into a large balloon. Assuming that all of the carbon dioxide ends up in the balloon, what is the volume of the balloon at 27 ∘C and a pressure of 735 mmHg ? Express your answer to three significant figures.

According to the ideal gas law, a 10.24 mol sample of xenon gas in a 0.8381 L container at 499.4 K should exert a pressure of 500.7 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a 4.194 L2atm/mol² and b 5.105×102 L/mol. Percent difference = |Pideal - Pvan der Waals x 100 Pideal + Pvan der Waals % 2