Asked by Amber
Could someone please help me start this problem?
The following reaction occurs 1.000 atmosphere & 298.0 K.
CH3OH (l) + 3/2 O2 (g) → CO2 (g)+ 2H2O (l)
50.00 g of CH3OH, and excess oxygen. Calculate ΔU using ΔU = ΔH - PΔV
The following reaction occurs 1.000 atmosphere & 298.0 K.
CH3OH (l) + 3/2 O2 (g) → CO2 (g)+ 2H2O (l)
50.00 g of CH3OH, and excess oxygen. Calculate ΔU using ΔU = ΔH - PΔV
Answers
Answered by
DrBob222
Calcuate dH with dHrxn = (n*dHo products) - (dHo reactants) and dH will be in kJ/mol. Then convert 50.0 g CH3OH to mols and calculate dH for the 50.0 grams.
Then calculate mols O2 initially and find the volume at the conditions listed, do the same for CO2 gas, find the difference and that is delta V. Then substitute and solve. Watch the sign on work.
Then calculate mols O2 initially and find the volume at the conditions listed, do the same for CO2 gas, find the difference and that is delta V. Then substitute and solve. Watch the sign on work.
Answered by
Amber
I got -1133.40 for the delta H and -19.07 for the change in volume, then put them in the equation.
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