What is the vapor pressure of benzene at its normal boiling point (80.1 °C)? Be sure your answer has the correct number of significant digits. mmHg x10 X 5

Oo.140. Subject:- Chemistry

For many purposes we can treat butane (C,H10) : as an ideal gas at temperatures above its boiling point of – 1. °C. Suppose the pressure on a 43.0 g sample of butane gas at 14.0°C is reduced to one-third its initial value. Oyes Is it possible to change the temperature of the butane at the same time such that the volume of the gas doesn't change? к10 no If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C.

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

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 550. L and heated to 520.0 °C. When the amount of CaCO3 has stopped changing, it is found that 8.46 kg have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 520.0 °C. Round your answer to 2 significant digits. P Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. 0 X

For many purposes we can treat ammonia (NH,) as an ideal gas at temperatures above its boiling point of –33. °C. Suppose the temperature of a sample of ammonia gas is raised from – 25.0 °C to 17.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.15 kPa and the volume decreased by 50.0%, what is the final pressure? Round your answer to 2 significant digits. kPa 1 Don't Know Submit etv DII esc %23 24 6 7 09 2 4 OP E T Y.

Calculate the total pressure (in atm) of a mixture of 0.0200 mol of helium, He, and 0.0100 mol of hydrogen, H2, in a 0.50 L flask at 10°C. Assume ideal gas behavior. Given that R = 0.0821 L'atm/(mol·K). a. 0.279 atm. b. 0.465 atm. c. 0.349 atm. d. 0.697 atm. O e. 1.39 atm.

Use your text or other reference to find the partial pressure of water at 25°C, 26°C, and 27°C and record those values.

Gaseous CO exerts pressure of 45.6 mmHg in a 56.0 L tank at 22°C was released to a room with a volume of 2.70 x 104L. The room has another two gaseous that are 5.50 g of NO2 and 8.034 x 1022 atoms of SO2 at 22°C. Calculate the partial pressure of CO in the room at 22°C. •Ans : P = 0.09458 mmHg Calculate the total pressure in the room and the molarity of CO gas in the room. •Ans: 5.14 x 10-6 M, Total pressure 2,7 x 10-4 atm Calculate the density of the mixture in the room and the mass percentage of SO2 gas in the room. 6.00027