A tank contains 10.6 g of chlorine gas (Cl₂) at a temperature of 84 °C and an absolute pressure of 6.00 x 105 Pa. The mass per mole of Cl₂ is 70.9 g/mol. (a) Determine the volume of the tank. (b) Later, the temperature of the tank has dropped to 32 °C and, due to a leak, the pressure has dropped to 3.00 x 105 Pa. How many grams of chlorine gas have leaked out of the tank?

A tank contains 10.6 g of chlorine gas (Cl₂) at a temperature of 84 °C and an absolute pressure of 6.00 x 105 Pa. The mass per mole of Cl₂ is 70.9 g/mol. (a) Determine the volume of the tank. (b) Later, the temperature of the tank has dropped to 32 °C and, due to a leak, the pressure has dropped to 3.00 x 105 Pa. How many grams of chlorine gas have leaked out of the tank?

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

See similar textbooks

Similar questions

A bubble of air is rising from the sea floor, from a depth of about 500 m. At this depth the pressure is 5.1*106 Pa (about 50.3 atm) and is at a temperature of about 7.0° C. It rises to the surface with the atmosphere, at a temperature of 20° C. If the bubble is observed to have a volume of 4 cm³ at the surface, what was its volume at the sea floor? Assume the number of moles of gas in the bubble is constant. B.
If a 5 m3 of gas initially at STP is placed under a pressure of 3 atm, the temperature of the gas rises to 17◦C. What is the volume now? Calculate to 2 decimals.
A small bubble rises from the bottom of a lake, where the temperature and pressure are 8°C and 6.4 atm to the water’s surface where the temperature is 25°C and the pressure is 1.0 atm. Calculate the final volume (in m3) of the bubble if its initial volume was 2.1 cm3.
If a 3 m3 of gas initially at STP is placed under a pressure of 2 atm, the temperature of the gas rises to 22◦C. What is the volume now? Calculate to 2 decimals.
We know from Newton's Law of Cooling that the rate at which an object warms up is proportional to the difference between the ambient temperature of the room and the temperature of the object. The differential equation corresponding to this situation is given by y' = k(M – y) where k is a positive constant. The solution to this equation is given by y = M + (yo – M)e-kt , where yo is the initial temperature of the object. Suppose your Thanksgiving turkey is kept at a temperature of 40 degrees Fahrenheit until it is put into a 350 degree Fahrenheit oven. It takes 2 hours for the turkey to warm up to a safe eating temperature of 165 degrees Fahrenheit. Find the values of yo, M, and k, for this situation, rounding your answers to 3 decimal places. Yo= M = k= Regardless of your answers above, suppose the k value in this situation is k = 0.3. Find the initial rate of increase of the turkey's temperature as soon as it is placed in the oven. Round to 3 decimal places. degrees per hour.
The temperature at a point (x, y) on a flat metal plate is given by T(x, y) = 96/(2 + x² + y2), where T is measured in °C and x, y in meters. Find the rate of change of temperature with respect to distance at the point (1, 3) in the x-direction and the y-direction. (a) the x-direction 1 °C/m (b) the y-direction Need Help? Read It °C/m Show My Work (optional) W S 3 E D $ 4 R LL % O G F7 A H FA * ( 9 ) O 4x D 7:16 PM 10/3/2022 Backspace
The pressure, volume, and temperature of a mole of an ideal gas are related by the equation PV = 8.31T, where P is measured in kilopascals, V in liters, and T in kelvins. Use differentials to find the approximate change in the pressure if the volume increases from 10 L to 10.6 L and the temperature decreases from 335 K to 330 K. (Note whether the change is positive or negative in your answer. I Round your answer to ti decimal places.
The volume of an automobile tire is 2.5 × 10−2m3 . the pressure of the air in the tire is 3.3 atm and the temperature is 17C ◦ . what is is the mass of air in grams ? The mean molecular mass of air is 29g. 1 atm = 1.01 × 105 Pa ; Calculate to 2 decimals.
VRMS-1 Consider a container of Argon gas at a temperature of 25.0 °C. The mass of an Argon atom is 39.96 AMU, where 1 AMU = 1.66×10-27 kg. (a) What is the average kinetic energy per Argon atom, in Joules (J)? (b) What is the RMS average speed of the Argon atoms, in meters per second (m/s)? (c) What would the temperature of the gas have to be for the RMS average speed to 275 m/s? Give your answer in degrees Celsius (°C).
According to the Ideal Gas Law, PV = kT, where P is pressure, Vis volume, T is temperature (in Kelvins), and k is a constant of proportionality. A tank contains 2000 cubic inches of nitrogen at a pressure of 26 pounds per square inch and a temperature of 600 K. Determine the EXACT value of k.
If a 3 m3 of gas initially at STP is placed under a pressure of 2 atm, the temperature of the gas rises to 22◦C. What is the volume now? Calculate to 2 decimals.
If a 2 m3 of gas initially at STP is placed under a pressure of 2 atm, the temperature of the gas rises to 63◦C. What is the volume now? Calculate to 2 decimals.