calculate U and H when the pressure of 0.02 mol of an ideal gas at 2 bar and 0.25 L is reduced to 1 bar and 0.25 L.
calculateU andH when the volume of 0.02 mol of an ideal gas at 1 bar and 0.25 L is increased to 1 bar and 0.50 L.
calculateU andH when 0.02 mol of an ideal gas at 2 bar and 0.25 L is expanded to 1.0 bar and 0.50 L isothermally.
calculate U and H when the pressure of 0.02 mol of an ideal gas at 2...
a 0.25 mol sample of a monatomic ideal gas is subjected to a pressure change of 4.0 to 0.50 atm in a constant volume of 2.0 L. what is the delta H for this process?
Assume there's 1 mol ideal mono-atomic gas in a 22.4L container at 300K. The initial entropy of the system is 100J/K. For the following processes, calculate: a) q and w for a reversible expansion to twice the volume, isothermally. b) S and G for irreversible isothermal expansion against a constant 0.5 bar external pressure, to a final internal pressure of 0.5 bar. c) U and H for adiabatic reversible expansion to twice the volume.
EXAMPLE 6-11 Applying the Ideal Gas Equation to a Mixture of Gases What is the pressure, in bar, exerted by a mixture of 1.0 g H2 and 5.00 g He when the mixture is confined to a volume of 5.0 L at 20 °C? Analyze For fixed T and V, the total pressure of a mixture of gases is determined by the total number of moles of gas: Ptot = ntotRT/V. Solve ntot = (1.0g Hz x 1 mol Hy)...
Vol calculate mol sample of an ideal gas expands reversibly and isothermally to a final OL If the initial pressure is 7.0 am and the temperature is 57.0°C (a) the initial volume of the gas (b) the final pressure of the gas (c) the work done in kJ (5) A 2 50 mol sample of an ideal monoatomic gas at 300K expands adiabatically and reversibly from a volume of 15.0 L to 60.0L Calculate the (a) final temperature of the...
4. (25pts) 20L nitrogen gas is compressed in a tank at 10 bar and 25°C. Calculate the maximum work (in joules) that can be obtained when the gas is allowed to expand reversibly to a pressure of 1 bar; (a) (10pts) isothermally (b) (15pts) adiabatically The molar heat apacity of nitrogen at constant volume is 20.8 J/K mol. Assume that nitrogen behaves as an ideal gas 4. (25pts) 20L nitrogen gas is compressed in a tank at 10 bar and...
1. a) One mole of an ideal gas at 298.15 K is expanded reversibly and isothermally from 1.0 L to 15 L. Determine the amount of work in Joules. b) Determine the work done in Joules when one mole of ideal gas is expanded irreversibly from 1.0 L to 15.0 L against a constant external pressure of 1.0 atm.
0.780 mol of an ideal gas, at 51.01 °C, is expanded isothermally from 1.94 L to 3.14 L. 1. What is the initial pressure of the gas, in atm? 1.07×101 atm You are correct. 2. What is the final pressure of the gas, in atm? 3. How much work is done on the gas, (in J), if the expansion is carried out in two steps by changing the volume irreversibly from 1.94 L to 3.14 L against a constant pressure...
1.0 mole of N2, 0.75 mol O2, and 0.50 mol H2, each at 25°C and 2 bar, are mixed isothermally. The final pressure is 2 bar. Calculate ∆S and ∆Ssurr, on the assumption of ideal behavior.
For the following processes, calculate the indicated quanti- ties for a system consisting of 1 mol of N2 gas. Assume ideal gas behavior. a. The gas, initially at 10 bar, is expanded tenfold in volume against a constant external pressure of 1 bar, all at 298 K. Calculate q, w, ?U and ?H for the gas. b. After the expansion in part (a), the volume is fixed, and heat is added until the temperature reaches 373 K. Calculate q, w,...
If 33.5 mol of an ideal gas occupies 87.5 L at 13.00 °C, what is the pressure of the gas? < Feedback The ideal gas law is pressure: presure: 6832 6832.2 PV = nRT When using 0.083145 L bar/mol K) as the value of R, the pressure (P) must be in bar, the volume (V) must be in liters, and the temperature (T) must be in kelvins. The symbol n represents the number of moles of gas. Rearrange the ideal...