Under adiabatic conditions you let a mass of gas expand by reducing the pressure on it. What happens to the temperature of the gas?
Under adiabatic conditions you let a mass of gas expand by reducing the pressure on it....
A monatomic ideal gas at room temperature undergoes an adiabatic process such that its final pressure is 3.75 times its initial pressure. a) Did the gas expand or contract? (b) What is the ratio of its final volume to its initial volume? A monatomic ideal gas at room temperature undergoes an adiabatic process such that its final pressure is 3.75 times its initial pressure. (a) Did the gas expand or contract? o expand o contract (b) What is the ratio...
an ideal gas expands to twice its volume under the following conditions: (a) isothermal; (b) adiabatic; (c) isobaric sketch each process on a PV diagram. In which case is the final temperature the greatest?
An ideal monatomic gas initially has a temperature of T and a pressure of p. It is to expand from volume V1 to volume V2. If the expansion is isothermal, what are thefinal pressure pfi and the work Wi done by the gas? If, instead, the expansion is adiabatic, what are the final pressure pfa and the work Wa done by the gas? Stateyour answers in terms of the given variables.
Air enters an adiabatic nozzle under the following conditions: pressure = 900 kPa temperature = 560°C velocity = 2.7 m/s The air leaves the nozzle at 850 kPa and 480 °C. What is the velocity at the exit of the nozzle? Assume the specific heat is constant and can be taken at the average temperature between the inlet and outlet. air (c) EYES Niel Crews, 2013
18. Under conditions of constant temperature and pressure, one mol of any gas will A. never occupy the same volume B. always react with 2 moles of gas C. alter its volume based on the molarity D. always occupy the same volume 19. what is the molar volume of a gas? A. it is the molar mass of an ideal gas. B. it is the volume of one mol of gas. C. it is the number of grams per volume...
e what happens under varying conditions. An ideal gas occupies a volume of 1.0 cm' and is at 20.0°C and atmospheric pressure. a. Determine the number of molecules contained in the gas. b. If the pressure is reduced to 10" Pa (a very good vacuum) while the volume and temperature remain constant, how many moles of gas remain in the container? c. Calculate the average speed of the nitrogen molecules in the gas.
1. what is the volume of a gas in linters under the following conditions, 4.59 mol of gas, with a pressure of 1.09 atm at a temperature of 35 degrees C. 2. what is the pressure of a gas in atm under the follwing conditions? 32.6 g of chlorine gas, at a temperature of 398 K, whose volume equals 1.62 Liters.
The density of a gas under NORMAL conditions (STP, 273K and 1atm) is 2.4 grams/Liter. There is an ideal gas inside a 20L volume container at a temp of 5 degrees celcius. The gas is allowed to leave the container, causing the pressure inside to decrease by 0.85 atm. (the temperature inside remains constant). What is the mass of the gas that is released?
Under constant-pressure conditions a sample of hydrogen gas initially at 73.00 degree C and 9.40 L is cooled until its final volume is 1.70 L. What is its final temperature?
Under constant-pressure conditions a sample of hydrogen gas initially at 112°C and 9.6 L is cooled until its final volume is 6.4 L. What is its final temperature (in °C)?