A cylinder container has a couple of holes punched into the bottom of it and the water is spurting out the holes due to the water pressure. You drop the water filled cylinder and as it is free falling the water no longer spurts out the holes.
What happens to g, and hence weight, and hence weight density, and hence the pressure in the reference frame of the falling container?
Could use an simple yet logical explanation of what happens in this scenario and also answers to the questions.© BrainMass Inc. brainmass.com October 24, 2018, 7:36 pm ad1c9bdddf
We can think of an simple example. Assume there are two cars chasing on the highway. Both cars have the same speed and acceleration and therefore, the relative speed between these two cars is always zero and the distance between these two cars is always a constant. If you are in one of ...
This solution provides briefs explanations of general physics concepts, including gravity, weight, and pressure.
What is the temperature of 0.52mol of gas at a pressure of 1.3atm and a volume of 11.7L ?
This figure (Figure 1) shows a container that is sealed at the top by a movable piston. Inside the container is an ideal gas at 1.00 atm , 20.0 ∘ C , and 1.00 L . This information will apply to all parts of this problem A, B, and C.What will the pressure inside the container become if the piston is moved to the 2.00 L mark while the temperature of the gas is kept constant?
A weather balloon is inflated to a volume of 29.0L at a pressure of 744mmHg and a temperature of 31.3 ∘ C . The balloon rises in the atmosphere to an altitude, where the pressure is 360mmHg and the temperature is -14.1 ∘ C.Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude
Calculate the density of oxygen, O 2 , under each of the following conditions:•STP
•1.00 atm and 25.0 ∘ C
To identify a diatomic gas (X 2 ), a researcher carried out the following experiment: She weighed an empty 1.0-L bulb, then filled it with the gas at 1.30atm and 26.0 ∘ C and weighed it again. The difference in mass was 1.5g . Identify the gas.
A 1-L flask is filled with 1.25g of argon at 25 ∘ C . A sample of ethane vapor is added to the same flask until the total pressure is 1.05atm .What is the partial pressure of argon, P Ar , in the flask?What is the partial pressure of ethane, P ethane , in the flask?
Imagine that you have a 7.00L gas tank and a 3.00L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 125atm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases.
13.0 moles of gas are in a 3.00L tank at 20.9 ∘ C . Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are a=2.300L 2 ⋅atm/mol 2 and b=0.0430 L/mol .
To prevent tank rupture during deep-space travel, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 4.00mol of gas D measured at 251 ∘ C in a 1.75-L container assuming ideal behavior?
To prevent tank rupture during deep-space travel, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 4.00mol of gas D measured at 251 ∘ C in a 1.75-L container assuming real behavior?View Full Posting Details