Dichloromethane is produced from two successive chlorination reactions: the chlo

Question

Dichloromethane is produced from two successive chlorination reactions: the chlorination of methane to methyl chloride followed by the chlorination of methyl chloride to dichloromethane: Using the standard heats of formation in the back of your text and the heat of reaction listed above, what is the standard heat of formation of CH2Cl2(l)? What is the standard heat of reaction for the combined (overall) reaction below? If methane and chlorine reacts to produce 336.0 mol/hr of CH2Cl2(l), and the reactants and products are at 25 degree C and 1 atm, how much heat is evolved or absorbed in the process? (Put the appropriate sign in your response and also indicate if the sign of your response means heat is evolved or absorbed.) __ Is this heat evolved or absorbed in the process?

Explanation / Answer

CH3cl(g)+ Cl2(g)-----> CH2Cl2(g)+HCl(g   DHrxn = -134.69 kj/mol

DHrxn = DHfCH2Cl2 +DHfHCl - DHfCl2 + DHfCh3cl

-134.69 =DHfCH2Cl2 + -92.31 - 0 + -82

DHfCH2Cl2 = enthalpy offormation of CH2Cl2 =   -145 kj/mol

2.
CH4(g) +2Cl2(g) -------> CH2Cl2(g)+ 2HCl(g)
DH0 rxn = (-145 +2*-92.31) - (2*0 + -74.8) = ?254.82 kj/mol

3. at standard conditions 298 k 1atm

CH4(g) +2Cl2(g) -------> CH2Cl2(g)+ 2HCl(g)

DRxn = ?254.82 kj/mol

336 mol/hr --- ?

Heat is evolved in the reaction    =   -254.82*336
= -85619.52 kj/ hr

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