Recent content by cheme101

You're on the right track. You have two unknowns, ΔH & ΔS - they should remain constant at all temperatures within the given range (hence the "average" specification). So you need two equations, at minimum. If you repeat your calculation for another temperature, that will give you (where d =...

Sounds like you're dealing with some kind of vaporizer. There are two things that heat can do when you add it to a liquid system: -if the liquid is below its saturation temperature (i.e. boiling point), added heat will increase the liquid temperature (Q = mcpdT). -once the liquid reaches its...

For 2 to 3: Isochoric Cooling - Const Volume. ΔU = NCvΔT = Q + W. W = PΔV so W = 0. ΔU = Q = NCvΔT. ΔH=ΔU+Δ(PV)=ΔU+VΔP

For 1 to 2: ΔG = ΔH - TΔS ΔA = ΔU - TΔS ΔU=NCvΔT=0 ΔH=NCpΔT=0 so ΔA = ΔG=-TΔS; you know T but need to find ΔS. There are two derivations; either will work for you. I'm going fast so may have mixed up negative signs & numerators/denominators, you need to double check the math when you do it...

I think you need to get into the thermodynamic partial derivative definition of these processes, i.e. Gibbs Energy: dG = -SdT + VdP Helmholtz Energy: dA = - SdT - PdV Now you set the appropriate terms to zero. i.e. adiabatic: is it a reversible process? isothermic: dT=0 isobaric...

I don't quite follow your table, but here's a general solution. For rate laws, the equation relating k to temperature is k = A * exp(-ΔE/RT). So you need to use your existing data and fit it to the equation by finding the constants A & ΔE (A is an arbitrary constant & ΔE is the activation...

You're on the right track, you just need to get your units right. Your slope (-ΔH/R) has to be in K because your x-coordinates are in 1/K; their product needs to be dimensionless to agree with ln(P). With consistent units: lnP = -(H/R)*T [unitless]= -([J/mol] / [J/mol K]) * (1/K) So if...