Recent content by Ariel Jo

q(gained by water)=q(lost by steam), and at constant pressure this would be q=n*Cp*deltaT for both substances. Setting them equal to each other would give moles of each, but there are no calculations to get 100degC as the equilibrium temp, just the (seemingly sound, but I'm not a physics...

Homework Statement You have 0.50 mol of steam which has been supercooled to 95˚C at 1 atm. Since the steam is below the boiling/condensation point, it proceeds to partially condense into liquid water. This happens in a thermally-insulated vessel at constant pressure. (a) When the system...

Would it look something like: ΔH500=ΔHo+(500-298)*___kJ/mol*___mol for each component of the reaction? Where ___kJ/mol is the molar heat capacity at constant pressure, and ___mol is the quantity of substance

Yup! The sum of the state functions of the products minus the sum of the state functions of the reactants is equal to the sum of the state function of the reaction; change in enthalpy is a state function, so it applies here.

Thank you! I will try the enthalpy=energy+pv equation. in (c) it was meant to be delta H, I've edited it so it should appear now.

Homework Statement For the reaction CH3OH(l) → CH4 (g)+ 1/2 O2 (g)[/B] (a) Calculate ∆Ho298 (b) Calculate ∆Eo298 (c) Write an equation that would allow you to determine ∆H at 500°C and 1atm Homework Equations ∆H=∆E+∆(PV) ∆H=Σ∆Hproducts-Σ∆Hreactants The Attempt at a Solution a)...