Question

a. Calculate the work (in kJ) when 2.50 moles of methane react with excess oxygen at 387 K:
CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l)

b. What is the approximate specific heat in J/(g^oC) of a metal whose M.W. is 63.7 g/mol? ( 253.6 g of water is in a Styrofoam calorimeter of negligible heat capacity. The initial T of the water is 21.5^oC. After 188.2 g of an unknown compound at 96.6^oC is added, the equilibrium T is 35.0^oC. The specific heat of unkown compound is 1.23411).

Answer 1

CH4(g) + 2O2(g) ----- > CO2(g) +2H2O(L)

since 2.5 MOLES OF METHANE will react with 5 MOLES OF O2 AND 2.5 MOLE OF CO2 AND 5 MOLES OF H2O ARE formed.

WORK DONE=P*DELTA V =DELTA N *R*T

WHERE DELTA N= CHANGE IN NO. OF GAS MOLES of product - moles of gaseous reactant =-5

WORK DONE=-5*8.314*387=-16087.59 J or -16.08 kJ/mol

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