An instrument, maintained at 165.2 °C, has two separate flasks that contain different gases. If the flasks are opened so that the gases are able to mix, what is the final density in flask 2? 2 Flask Gas Pressure (atm) Volume 1 C6H8 2.5 4.4 2 C4H8O2 6.4 5.8

For many purposes we can treat dimethyl ether (C₂H₂O) as an ideal gas at temperatures above its boiling point of -24. °C. Suppose the pressure on a 15.0 g sample of dimethyl ether gas at - 12.0°C is cut in half. Is it possible to change the temperature of the dimethyl ether at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. yes no [°C x10 X Ś

Calculate the root mean square speed of Xe gas at 50.0 °C. 7.83 m/s 24.6 m/s 97.5 m/s 248 m/s 6.14 x 104 m/s

If 85.6 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and decompose completely via the equation below, what would be the final pressure of carbon dioxide (in atm) assuming it had the full 2.00 L in which to expand? H₂CO3(aq) → H₂O(1) + CO₂(g)

What is the partial pressure of O2 in the mixture?

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

If 51.2 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and decompose completely via the equation below, what would be the final pressure of carbon dioxide (in atm) assuming it had the full 2.00 L in which to expand? H₂CO₃(aq) → H₂O(l) + CO₂(g)

If 58.4 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and decompose completely via the equation below, what would be the final pressure of carbon dioxide (in atm) assuming it had the full 2.00 L in which to expand? H₂CO₃(aq) → H₂O(l) + CO₂(g)

If 76.6 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and decompose completely via the equation below, what would be the final pressure of carbon dioxide (in atm) assuming it had the full 2.00 L in which to expand? H₂CO₃(aq) → H₂O(l) + CO₂(g)