Twenty-five milliliters of liquid nitrogen (density = 0.807 g/mL)is poured into a cylindrical container with a radius of 10.0 cm anda length of 20.0 cm. The container initially contains only air at a pressure of 760.0 mmHg (atmospheric pressure) and a tempera-ture of 298 K. If the liquid nitrogen completely vaporizes, what is the total force (in lb) on the interior of the container at 298 K?

You collect butane gas in a graduated cylinder that is inverted and partially filled with water. There will be water vapor present in the gas. If the total pressure inside the graduated cylinder is 747.8 torr and the temperature is 25, what is the vapor pressure of just the butane gas?

A sample of oxygen is collected over water at 24°C and 757 mm Hg in a 125-mL flask. The vapor pressure of water at 24°C is 22.4 mm Hg. The partial pressure is 734.6 mmHg. There are 4.96x10^-3 moles of dry gas collected. If 0.0205g of N2(g) are added to the flask at the same temperature, the partial pressure of nitrogen in the flask is 108.7 mmHg. What is the total pressure in the flask after nitrogen is added?

Suppose a volatile liquid is completely vaporized into a 157 mL flask in a 99.1°C boiling water bath. What is the molar mass of the volatile liquid if the corrected mass of the condensed vapor is 0.299 g and the final partial pressure of air in the flask is 687 mm Hg?

. A 4.25 g sample of the refrigerant Freon -12 is vaporized and found to occupy  a volume of 1.36 L at a temperature of 50 degrees celcius and a pressure of 521 mm Hg. What is the molar mass of Freon -12degrees celcius?

In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. Lithium hydroxide, LİOH, is used in spacecraft to re-condition the air by absorbing carbon dioxide exhaled by astronauts as shown in the reaction: 2 LIOH(s) + CO2(g) → Liz CO3(s)[+ H2O(1) What volume of carbon dioxide gas at 21.0 °C and 781 mm Hg could be absorbed by 327 g LIOH? Enter your value in the first box and an appropriate unit of measure in the second box.

Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial chemical, and world production exceeds 2.0 × 10¹¹ kg per year. The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces 3.1 kg of solid sulfur and 10.0 atm of oxygen gas at 800. °C into an evacuated 70.0 L tank. The engineer believes K = 0.98 for the reaction at this temperature. Calculate the mass of solid sulfur he expects to be consumed when the reaction reaches equilibrium. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken in his belief about the value of K, and the consumption of sulfur you calculate may not be what he actually observes. p' kg ☐ x10 ×

When collecting a gas over water it is necessary to correct for the vapor pressure of water in order to determine the pressure of the gas you are collecting. We will do this by using a graph of ln P in mmHg versus 1/T where T is the temperature in Kelvin. The equation is y = -5206.4 x + 20.621 (With an R^2 = 0.9999). If you collect a gas at 26.8 ℃, what is the value of “x” that you want to use in the equation. (Keep the answer for the next question). (Keep extra digits, you do not want to round in the middle of this calculation). Select one:   a. 0.003660992 b. 0.037313433 c. 0.003378378 d. 299.95 e. 0.0273150 f. 273.15 g. None of these h. 0.003333889 i. 0.0027315

A sample of oxygen gas was collected via water displacement. Since the oxygen was collected via water displacement, the sample is saturated with water vapor. If the total pressure of the mixture at 26.4 °C is 737 torr, what is the partial pressure o oxygen? The vapor pressure of water at 26.4 °C is 25.81 mm Hg. torr