constant pressure gas thermometer problem delta h

The pressure of a gas is 100.0 kPa and its volume is 500.0 ml. If the pressure is decreased to 0.75 atm, what is its new volume? 2. The volume of a gas is 10.0 liters and its pressure is 1.5 atm. I've tried using the ideal gas law: PV=nRT but i can't seem to get where I am getting lost.

If we took 2.00 liters of gas at 1.00 atm and compressed it to a pressure of 6.00 x 104 atm, what would the volume of that gas be?Ĭalculate the Volume occupied by 1.5 moles of an ideal gas at 25 degrees Celsius and a pressure of 0.80 atm. Synthetic diamonds can be manufactured at pressures of 6.00 x 104 atm. The volume of the container is then reduced to half its original volume. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a pressure of 0.724 atm, and N2O4 at a pressure of 0.0524 atm. I got this answer by plugging in the values into the equationĬonsider the following reaction. What is the final pressure exerted by the gas? 1. I will be happy to critiqueĪ 0.65 mole quantity of O2 occupies 4.0 L at 20.◦C. If I raise the temperature to 350K and lower the pressure to 1.5 atm, what is the new volume of the gas? Use the combined gas law here. w = _ J now calculate the work done if thisĪ gas takes up a volume of 17 liters, has a pressure of 2.3 atm, and a temperature of 299K. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 20.0 L. (a) What is the temperature when the pressure is 0.0500 atm? �C (b) What is the pressure atĬonsider an ideal gas encloesd in a 1.00 L container at an internal pressure of 10.0 atm. The pressure in a constant-volume gas thermometer is 0.700 atm at 100�C and 0.512 atm at 0�C.

Constant pressure gas thermometer problem delta h