I need help with problem 4. I have included problems 7-4, 8-7, and problem three

Question

I need help with problem 4. I have included problems 7-4, 8-7, and problem three for reference.

4. Deduce the balanced reaction in which synthe- sis gas is formed by combining equal volumes of methane and carbon dioxide. From enthalpy of formation data given in Problems 7-4 and 8-7 decduce the enthalpy change for this reaetion. By applying Le Châtelier's principle, deduce whether the conversion of the gases to carbon monoxide and hydrogen will be favored by low or by high pressures, and by low or by high temperatures. Combining these results with those obtained in Additional Problem 3, determine the fraction of

Explanation / Answer

the reaction is CH4+CO2----->2CO+ 2H2

standard heats of formation ( KJ): CO= -110.5, CO2= -393.5 and CH4=-76, H2=0

enthalpy change ,deltaH= sum of standard heat of formation of products- sum of standard heat of formation of reactants =

2*(-110.5)+ 0- {-76+(-393.5)}=248.5Kj

standard entropy (J/mole.K) : CO=197.6, H2=130.6, CO2=213.6 and CH4=186.2

entropy change, detlaS = 2*197.6+2*130.6- (213.6+186.2) =256.6 J/K

standard gibbs free eneergy change= deltaH-T*deltaS= 248.5- 298*256.6/1000 Kj=172 KJ

since deltaG is +ve, the process is not spontaneous. since deltaH is +ve, the reaction is endothermic and increased temperature as per lechatlier principle favors the backward reaction to compensate the effect of temperature increases. So low temperarues are preferred.

there are more moles on products than reactants. Since decreased pressure favors the forward reaction.

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