One mole of a gas is expanded from 0.1 bar to 0.01 bar at a constant temperature of 350 K. The gas obeys the equation of state p(Vm - b) = RT where b is a constant equal to 0.01 dm3 mol-1. Find ΔH in mJ for this process.
One mole of a gas is expanded from 0.1 bar to 0.01 bar at a constant...
Because (∂H/∂P)T =−CPμJ−T, the change in enthalpy of a gas expanded at constant temperature can be calculated. To do so, the functional dependence of μJ−T on P must be known. Part A Treating Ar as a van der Waals gas, calculate ΔH when 1 mole of Ar is expanded from 329 bar to 1.68 bar at 375 K. Assume that μJ−T is independent of pressure and is given by μJ−T=[(2a/RT)−b]/CP,m, and CP,m=5/2R for Ar. The van der Waals parameters a...
One mole of O2(g), with CV,m=2.5R, is expanded adiabatically from 301 K and 4.00 bar to 1.60 bar against a constant external pressure equal to the final pressure. Calculate q, w, ΔU, ΔH, ΔS and ΔSsurr. Enter your answers in the specified units with three or more significant figures . Do not include units as part of your answer. q = ____________ J w = ____________ J ΔU = ____________ J ΔH = ____________ J ΔS = ____________ J mol-1 K-1...
One mole of an ideal monatomic gas is expanded from an initial state at 3 bar and 450 K to a final state at 2 bar and 250 K. Choose two different paths for this expansion, specify them carefully, and calculate w and q for each path. Calculate ?U and ?S for each path.
8. Initially, 1 mole of the real gas is contained in a thermally insulated piston-cylinder arrangement in an initial state (T1, P1, Vi ). 1 mole of the real gas that is expressed by the following equation of state under the investigation. Now, the gas is expanded so as to fill the final state of (T2, P2, V2 ). Suppose that any possible temperature dependence of Cy is negligibly small and the molar heat capacity is approximately equal to 2"...
3. A mole of perfect Gas initially at 101 325 pa is expanded from 22.4 L at a constant pressure of 0.20 bar at a constant temperature of 273 K until it cannot expand anymore. Is this expansion spontaneous? How much heat is transferred in this process? How much has the entropy changed as a result of this process?
For the 2.50 mole sample of the gas with the equation of state given The gas is described by the equation of state PV=n(RT+PB)where B = 82.0 cm3/mole. expand the gas from 20.0 bar to 2.00 bar isothermally at 500 K, and calculateΔA and ΔG.
One mole of a monatomic ideal gas expands from 4 to 10 L at constant pressure of 1 atm. Assuming that Cp = 20.8 J/mol-K, calculate ΔH for this process.
Atomic gas which obeys Van der Waals equation of state RT= (P+ a/ V2) (V-b) has internal energy (per mole) of u = 3/2 RT - a/V where 'V' is volume of mole in temperature T. In the beginning, the gas temperature is T1 and volume V1. The gas is let to expand adiabatically so that its final volume is V2. What is the final temperature of the gas?
I. (30 pts.) One mole of an ideal gas with constant heat capacities and ? 5/3 is compressed adiabatically in a piston-cylinder device from T1-300 K, pi = 1 bar to p2 = 10 bar at a constant external pressure Pext"- P2 -10 bar. Calculate the final temperature, T2, and W, Q. AU, AH for this process. 2. (20 pts.) Repeat problem 1 for an adiabatic and reversible compression. 3. (20 pts.) A rigid, insulated tank is divided into two...
One mole of an ideal gas with CP = (7/2)R and CV = (5/2)R expands from P1 = 8 bar and T1 = 630 K to P2 = 1 bar. Take the value of R as 8.314 J·mol-1·k-1. At constant volume (assume mechanical reversibility), find the value of W, Q, ΔU, and ΔH? rt.)