If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas?

If I have an unknown quantity of gas held at a temperature of 370 K in a container with a volume of 33.4 L and a pressure of 9.02 atm, how many moles of gas do I have?

If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? Hint: Use ideal gas law, PV=nRT, and the universal gas constant R=0.0821 L*atm/K*mol.

Problem 1: Consider the two-sided chamber shown,where the right half has a volume of V = 590 L and the left half has a volume of 2V. The chamber has a seal which separates the right from the left half. The chamber is sealed and an ideal gas is pumped into the right side at a pressure P= 6.4 atm and temperature T= 78° C. The seal between the two sides is then opened. 2V V Part (a) If the physical temperature decreases by a factor of 2 while the gas fills the chamber, what is the new pressure, in kilopascals? P'= sin() cos() tan() 7 8 HOME cotan() asin() acos() 5 atan() acotan() sinh() 1 2 3 cosh() tanh() cotanh() + END ODegrees O Radians Vol BACKSPACE CLEAR Submit I give up! Hint Feedback Part (b) The chamber is then sealed again, trapping 2/3 of the gas molecules in the left side. The temperature of the left side is then doubled, back to the original temperature T. What is the pressure in the left side of the chamber now, in kilopascals?

At standard temperature and pressure, a gas has a density of 0.085 kg/m3.  What volume (in m3) does 1.03 kg of hydrogen occupy at standard temperature and pressure

P1. Consider a gas of oxygen atoms (µo, = 32 g/mol). What should the temperature of the gas be for the mean square speed of the atoms to be v = 100 m/s? While keeping the temperature the same as before, what should the pressure of the gas be for a container of volume V = 51 to be able to contain m = 1 kg of oxygen? How much does the temperature of the gas increase if the container is dropped on the ground at a speed of u = 2 m/s? You may neglect thermal conduction with the outside.

A mass m of helium gas is contained in a container of constant volume V, with a pressure P and absolute (Kelvin) temperature T at the start. More helium is added, increasing the total mass of helium gas to 3 m. The temperature is found to be 2T after this addition. In terms of the initial pressure P, what is the final gas pressure?

A sealed  29.0-m3 tank is filled with  2,474 moles of oxygen gas (O2) at an initial temperature of 270 K. The gas is heated to a final temperature of  487 K. The ATOMIC mass of oxygen is 16.0 g/mol, and the ideal gas constant is R = 8.314 J/mol · K = 8.314 J/mol · K. The final pressure of the gas in kiloPascals is closest to

The number density of gas atoms at a certain location in the space above our planet is about 1.40 ✕ 1011 m−3, and the pressure is 1.10 ✕ 10−10 N/m2 in this space. What is the temperature (in °C) there?

A gas chamber is to be designed to separate two gases with the following specifications: Hot gas temperature 1145°C Cold gas temperature 45°C Hot gas heat transfer coefficient 230 W/m² K Cold gas heat transfer coefficient 290 W/m² K Metal wall thermal conductivity 115 W/m K If the maximum temperature of the wall on the hot side does not exceed 545°C, using thermal resistance concept, what thickness should the metal wall between the hot gas and cold gas be in mm?