One mol of an ideal, monoatomic gas undergoes a reversible adiabatic expansion from 1.15 L to 4.65 L starting at 400 K. Calculate q, w, delta U, delta H, and delta S.
Calculate the entropy change for heating H2O(s) at -10 degrees C to H2O(l) at 10 degrees C.
A sample of liquid benzene weghing 0.633 g is burned in a bomb calorimeter at 25 degrees C, and 26.54 kJ of heat are evolved. Calculate delta U and delta H
Calculate the entropy change when 100 g of argon is heated and compressed from 300 K, 1.0 atm, to 900 K, 17 atm, assuming ideal gas behavior. Cp=20.93 J/K mol
Consider the reacton: 2 H2(g) + O2(g) -------> 2 H2O(g). Determine delta G for this reaction at 1000 K.
Calculate deltaS standard for the sublimation of CO2. The enthalpy of sublimation is delta H^0=25.23 kJ/mol at 195K. delta S^0= 1 ATM
FIND THE ENTROPY CHANGE DELTA FOR ARGON GAS UNDERGOING THE FOLLOWING TEMPERATURE AND PRESSURE CHANGES: Ar(g),P=1 atm, T=300 K------> Ar(g), P=10 atm, T=500K
The heat capacity of a gas is given by Cp=a+bT where a and b are constants a) determine delta S for heating the gas from T1 to T2 at constant P b) determine delta G for heating the gas from T1 to T2 at constant P hint the integral lnx dx= x ln x-x
Show that the partial of H with respect to P at constant T =0 for an ideal gas.
Show that the partial of H with respect to P at constant T =0 for an ideal gas. Hint: start with dH=VdP+TdS. Divide by dP and impose constant T. Use a maxwell relation from dG.
Determine the delta G standard state at 298 K from the following standard state values at T= 298
Consider the combustion reaction for propane below. CH3CH2CH3(g)+5O2(g)-------->3 C02(g)+4H20(g) a) Determine the delta G standard state at 298 K from the following standard state values at T= 298 S(CH3CH2CH3)=269.9 J/K mol S(C02)= 213.7 J/K mol S(H20)=188.8 J/K mol S(02)=205.1 J/ K mol delta H(CH3CH2CH3)=-103.9 kJ/mol ...continues
