Use standard heat of formations to find the heat for the combustion of 5.0 g of...

Use standard heat of formations to find the heat for the combustion of 5.0 g of Methane gas CH4 to form carbon dioxide and water vapor

Expert Solution

BALANCED EQUATION : CH4(g) + 2O2(g) ---> CO2(g) + 2H2O(l)

DH0rxn = (1*DH0f,CO2 + 2*DH0f,H2O)-(1*DH0f,Ch4+2*DH0f,O2)

= (1*-393.5 + 2*-285.8)-(1*-74.81+2*0)

= -890.29 kj/mol

no of mol of CH4 burned = w/Mwt

= 5/16

= 0.3125 mol

1 mol CH4 = 815.48 kj

so that, heat released(q) = n*DHrxn

= 0.3125*890.3

= 278.22 kj

DHcomb = -278.22 kj

queen_honey_blossom answered 1 year ago

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